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>> ok, unit six, today, whichis the last unit before the next exam, right? it should be on wednesday. this is acid-base--acid-base theory. and there are different typesof acid-base theory depending on which area ofchemistry you're looking at. for example in ochem, organicchem, they're generally looking at lewis acids and bases. biochem and mostarea of general chem.
favor bronsted-lowry. and then we havearrhenius which is to a certain extent justhistorically important, ok? but we're looking atthe arrhenius definition and the bronsted-lowry. it's going to go alittle bit out of sequence with how it's presentedin the book. all the topics should be covered but i don't cover them quitethe same way that they are
in the book because i get-- the continuity isinterrupted a little bit. i talk about arrhenius thengo right into bronsted-lowry, not do arrhenius thatcalculate ph and do other things and then come back and starttalking about acid-base theory. so it's all in them. just understand that youmight have to jump back and forth a little bit. [ writing on board ]
ok, under the arrheniustheory, an acid is anything that produces h plusand so there's-- acid is anything that donatesor produces h plus in solution, and it's worth noting here that h plus is nothingmore than a proton, right? if we have h plus, welook at the hydrogen atom. this is a hydrogen atom, right, which actually doesn'texist in nature, right? it actually exists ash2, diatomic molecule.
we can make it though,we can make it real easy. if you go h plus that meansthat you have one less electron than the number of electronsrequired to be neutral which in this case, sincethere's only one proton, is itself one electron. so if you get rid of theone electron on hydrogen to create h plus you havenothing more than a proton. and the reason whyi tell you this is because the termsare synonymous.
so if you run into them inthe lab or other textbooks, h plus and protonare the same thing. and in reality, it doesn't existin an innocuous environment or that these free h pluses. if you took an acid and youevaporated all the water off the acid, you would not have abeaker full of protons, ok? the protons actually existonly as free protons, only in the gas based. in the laboratory,it actually exists
as a protonated watermolecule called hydronium ion. it's called hydronium. this is what we reallysee in the lab. and when we're talking aboutacids and bases, and protons and things like that, theseare terms that we used as a matter of convenience. in reality, this is how itexist, h3o plus hydronium, ok? notice, you know, this"oium" we saw it in ammonium. remember nh4+ was ammonium,
whenever you have a reasonablyelectronegative element like nitrogen oxygen,carrying a positive charge, it takes this oniumending just a little aside. ok, so i usually referto them as protons. ok, so an acid is aproton donor to solution, anything that producesprotons, h plus. this is arrhenius right? a base is anything thatproduces oh minutes ok, so these-- like i said thisstill have historical importance
and we still use themwhen we look at-- when we start calculatingphs and pohs. under the arrheniustheory, acid produce h plus, bases produce oh minutes, ok? cotton dry. but then you'd run intothings like ammonium nh3. this is a base. this is a base and you'resaying, what the heck. under the arrhenius definition,it's got to produce oh
and ammonia doesn'tany oxygen in it. so there were compoundsthat existed that were in apparent contradictionto the definitions presented in the arrhenius theory. in reality it was, still abase, i can show you just now but there's stillwere some thing that was caused for confusion. it turns out thatammonia does not ionized because remember wetalked about ionize.
it produces ions and solution. ammonia doesn't ionizedunless you add water to it and make it aqueous. once you add water to it,you get the following-- you get ammonium hydroxide whichquickly dissociates and ionizes into ammonium plus hydroxide. so there it is, ok? but again, this will onlyoccur if you have water in your ammonia solution.
everybody smelled ammonia. this is a cleaning solutionthat we use, you know, routinely clean floorsand stuff. and it's also one of thethings in smelling stuff. it wakes you up whenyou get knocked out. ok. so there were things thatdidn't at least on the surface, agree with the arrhenius. so two other guys bythe bronsted and lowry. some people just call this abronsted theory but i'm going
to give credit for lowry. this is a bronsted-lowry and bronsted is germani believe, i hope. bronsted-lowry definition,acid is the same. i mean look at thebronsted-lowry definition. the acid is exactly the same. anything that producesproton or donates proton to solution, produces h plus. the base is somewhat different.
bronsted-lowry describesthis base or a base under the bronsted-lowrydefinition is an h plus acceptor. anything that acceptsh plus is a base under the bronsted theory. now one consequence of bronsted-lowry was youcouldn't have without the other. you can't have onewithout the other. if you have a protondonor in solution,
you must have a proton acceptor. in fact it's actuallythe acceptor that defines the donor, ok? a proton donor does not becomea donor, until something in solution actuallyaccepts the proton. ok? it's very similar to adonation, you make the chair of organization like write 5,000dollar cheque, i'm going to, you know, stick it under thetire of the car, in your garage, it hasn't moved for threeyears and you go to your taxes
and you say, "no, no, no. i gave a 5,000 dollar donationto the united dog funders." and they said, "great,great, that's a write off. let me see the cancel cheque?" "well, i don't have them,i don't have that cheque." it doesn't become a donationuntil someone accepts it, same thing here, right? they define each other. so something veryinteresting results
from that particularrequirement in bronsted-lowry. so let's see if we have some. i can make them up but i don'tlike pointing, wait a minute. i must go through this stuffsince i'm going to [inaudible]. [ pause ] now, the one thing thatwill always be true, ok, when you see this, it's alwaysan acid, always, no exceptions. this is always acid andthis is always base. this will always be true.
you can't make too many ofthose statements in chemistry and have the words likealways and never in them. when you see h3oplus, it is acid. when you see oh minutes,it is base. the problem is, is thatyou don't always see them. there are examples ofreactions that don't contain h3o or oh minus but when you dosee him you can automatically label them. we can do the one we justhad up here, the ammonium.
so let's take a lookat an example in your book is aqueousplus water goes to-- i'm going to breakthis apart, ok? i'll write this again here. so i have this reactionand you won't-- you're not expected to comeup with these, all right, this would be more alongthe lines where it says, aqueous is chemical reaction. and what i want you to dois label every species,
every compound, neutral, or ionas either an acid or a base. now, this isn't asdifficult as it might seem because if you know one, you canget the other three according to the bronsted definition,bronsted-lowry. so, i'm looking atthis equation. is there anything that iknow 100 percent for sure? what? >> and [inaudible]the term oh negative. >> what about it?
>> oh negative is base. >> right, right here it is. i know for sure that oh isa base so i label it base. oh is a base. bronsted-lowry says you cannothave one without the other so the other one must be-- >> acid. >> acid, it's got to be. you can't have onewithout the other-- acid.
see the nitrogencontaining compound? it differentiates itself fromthe oxygen containing ion, these are-- put ionsin a compound. if the nitrogen containingspecies was an acid on this side, it's theopposite on the other side, it makes this a base, bronsted-lowry said itcan go on with the other. this must be an acid. does everybody see that?
it starts with identifyingonly a single species. once you get that one under yourbelt you can determine what all are the other ones are. everybody good? now, the acid on one side of thearrow, reactant, and the base on the other side have avery special relationship-- acid on one side,base on the other, acid on one side,base on the other. don't go acid, acid.
it's not acid, acid. it's acid, base, acid, base. everybody see that? these are calledconjugate acid-base pairs. called conjugateacid-base pairs. what's the differencebetween acid-base on one side, acid-base on the other side,what are they differ about it? you got nh3 on one side,nh4 plus on the other. you got oh minus on oneside and h2o on the other.
h2o you could think aboutis being this, right? hoh. we'll see thatin next lecture. ok. >> so they get [inaudible]one hydrogen plus. >> 1h plus right? conjugate acid-base pairsdiffer by the proton, the h plus that is transfer. let's see if ourdefinition according to bronsted-lowry make sense.
nh3 is a base which meansit is h plus acceptor. h20 in this case is an acid which means it'san h plus donor. h20 donates h plus to nh3. nh3 was neutral andjust took on h plus which means it's overall netcharge now has to be plus one and it's hydrogen one pop byone count, it makes sense right? this donated acid, thisaccepted base, make sense? let's see if it worksthe other way.
this is a base, this is an acid. nh4 plus defined as anacid has to donate h plus. if it donates, h plus, thishydrogen count goes down by one and because it waspositively charged then gave up the positive itgoes to neutral. the oh minus accepted the hplus, its hydrogen count went up one and the plus and minuscancel out, it went neutral. so they do make sense,go in both ways, right? it makes perfectsense going both ways.
now incidentally, an acid define under bronsted-lowry wouldbe an acid under arrhenius which would be anacid under lewis. ok? these different theoriesjust give you a different reference point for looking athow things are defined in terms of what is an acid,what is a base. but an acid under one wouldbe an acid under all of them. there's no conflict there. ok? let's do someother examples.
this concept of conjugateacid-base pairs, it's important and it's going to be importanteven in this lecture, ok? it's going to be importantwhen we get to buffers. it's going to beimportant when i ask you, "what is the conjugateacid of this? what is the conjugatebase of this?" so let's take a lookat another one-- we put aqueous >> h2o liquid, pure liquid.
what do we know for sure? >> the oh negative. >> oh negative is a-- >> base. >> base. bronsted-lowrysays cannot have one without the other. if that is the basethis must be an acid, the dihydrogen phosphate ionand look for something similar to the phosphate group.
on the other side, there it is. if this was an acid, itmakes it a base over here. bronsted-lowry says, you cannothave one without the other. that must be acid. identify the conjugateacid-base pairs-- i think the last examplewas the same way, right? number one was with numberthree, number two was with this four but thatwas just a coincidence. it's not always the first onehere it's going to be connected
to the first one on theproduct side and-- not so much. does everyone understand? yes? what is the conjugateacid of hco3 minus? >> h203? >> how do you know that? >> because it's-- wellthat's the [inaudible] so you're looking for an acidso you have to be to donate. let's say a nitrogen so youhave to add that [inaudible].
>> that's exactly how i wouldhave explained it too, exactly. maybe not word for wordbut that's exactly. if you're being askedfor the conjugate acid, what do you have? what were you given? >> debates. >> debates, right? debates that makes sense. they're not going to askyou for the conjugate acid
and then give youthe acid, right? so if you're being askedfor the conjugate acid, you're given the base,what do bases do? so you have to increasethis by h plus. adding h will do that. adding plus will cancelthe plus and minus, right? first of all you know. i mean you're going tosee this on the exam, 100 percent guaranteed.
not on the quizzes, on the exam. when you have thisand they want-- and you're asked what's aconjugate acid, conjugate base? you know that you're onlyhave two possibilities. there's only two possibleanswer here, this. without an h plus orthis with an h plus. so scratch out the other two because they're not evenpossibilities, right? the only two possibilities aretaking h plus away from that
or adding h plus to that. that's the only twopossibilities. so you can narrow itdown, just like that to 50-50, two answers, right? if you're asked for theacid, you're given the base, what the bases do exceptyou're going to increase. another-- students in thepast have said, "well, i think it's easierif you're asked for the conjugate acidto add, add h plus."
what is a conjugatebase of hso4 minus? [ inaudible remark ] you want to get that? no. get him at? got it? if you're asked forthe conjugate base, you must be given the-- >> acid, what do acids do? they donate h plus.
they produce h plusin the solution. so you're going to lose h plus which means thishydrogen is gone and since you'resubtracting h plus, it goes back down, negative 2. ok? you will be askedto do them. you'll be asked 100percent to do that. always remember, conjugateacid-base pairs only differ by h plus.
it only differ by h plus. if you see conjugateacid-base pairs which we will seen a little bit-- these are conjugateacid-base pairs because they differonly by h plus. it's real easy to figureout which one is the acid and which one is the base right, along with the greaternumber of hydrogen. they're only going todiffer by 1h plus along
with the greaternumber, the acid, the lesser number is base, ok? you're all expertsnow in the application of bronsted-lowry, all right? a consequence again of bronsted-lowry isconjugate acid-base pairs because of the requirementthat you have to protons donors and acceptors and solutionsat the same time, yeah. good. now there arevarying strengths
to the differenttypes of acids, ok? strong acids-- you got to write that straight. strong acids ionizednearly 100 percent. they ionized completely, ok? hcl is a strong acid, in aqueousenvironment in water, ok, there's a couple of differentways you can write this but it's the same thing-- or you could see it simplyas removing the water
because everybodyknows it's better. that's aqueous again. i cannot put a q. i can'twrite in cursive anyway. i'm trying to put a q afteran a, just doesn't happen. these are the same things. what's more complete,what's more accurate, this one becauseit shows the water, it shows the conjugateacid-base pairs, right? and in this case hclacid, base, acid, base,
but we could haveworked backwards, right? we could have said,this is acid right here because anytime we seeh3o plus is an acid. and besides, cl minushas to be a base, right? why? why does cl minushave to be a base? >> the other one is absolute. >> it's what? >> it's absolute. >> this is conjugatepairs in that.
>> yes. >> well, even more than that. let's look at even atmore and simpler terms. what do acids do? >> donate. >> donate what? >> an h. >> h plus. why does cl minushave to be a base?
>> it doesn't have-- >> it doesn't havean h plus does it? see, how there's no h plusthere, so it couldn't donate. this is base, acid. base. notice with the short-handversion which is done routinely as a matter convenience. it's a matter of convenience,it's done all the time that it's written this way. you can't identifyconjugate acid-base pairs
on this way, right? you can't do it. but hcl is a strong acid andyou know how i know it's a strong acid? it's on the list ofstrong acid in your book. that's the only way you knowif something is a strong acid. you memorize that list. how many are on this? six, eight, it depends onwhich book you look at.
usually there's six, right? yup, we have six. memorize them. it would be in your bestinterest to memorize them. strong acids ionize completely. that's what you alwaysthink in your mind when you hear theword strong acid, strong acid break apartvirtually 100 percent at the time.
that means if you havehcl, hydrochloric acid, we'll get to thenaming in just a minute. if you have hcl inwater, aqueous, hcl doesn't actually exist. the molecular formof hcl doesn't exist because every single oneof the hcl is broken apart into h plus and cl minus. all it is is a bunch of h plusesand cl minuses floating around. ok? now whether or not aparticular substance will be a
strong acid of a weak,we'll talk about weak in just a minute, is allrelated to how well the result in negative is establishedon the anion. now when you lose hplus, i don't care where you're starting from,you're going more negative. if you're at negative 3 andyou lose h plus you're going to negative 4. if you're neutraland you lose h plus, you're going to negative one.
if you're plus one and youlose h plus, you're going zero. so you're going more negative. how well the resulting anionis stabilized will determine whether or not that thingeven loses the h plus. so you look at chlorine,very electronegative ion, right under fluorine,all the allergens, group 7th are veryelectronegative, ok chlorine can handle anegative charge real well. so when it loses,hcl loses h plus.
the result in anionis already stable. ok, strong acids ionize 100percent, virtually 100 percent. and strong acids are identified because you memorize thelist of strong acids. because anything else thatis an acid that is not on that list is weak acid. so do you want to memorize, youknow, a hundred of weak acids? or do you want to justmemorize six strong and say, anything else that'san acid is a weak acid.
now do weak acids do? what's the first bigdifference you see between those two equations? and again you couldalso write this as-- ok, we'll separate right here,the line across here, so. hcl is a strong acid. i know that because i memorizedmy list of strong acids. i'm going to rewardingprobably tomorrow on the quiz if i memorize my list of strongacid, wink, wink, all right?
when i look at these two,what jumps out at you? >> equilibrium arrows. >> yeah, perfect. the equilibrium arrowshere, right? it appears that the weak acidhave reversible reactions, you know, in equilibrium, while the strong acidsdon't, and that's true. h plus will not recombine withcl minus and form molecular hcl. because we know thatmolecular hcl
and water disassociates almost100 percent at the time. basically they hate each other. and as soon as you give themwater, a vehicle for them to ride apart from eachother, they do it, they do it. i think one of he moreconcentrated forms of hcl, the 17 molar, that'svery concentrated. burn you quick. down here we have equilibrium. weak acids only partiallyionized, ok,
only partially ionized. that means weak acidsexist primarily as molecule in a molecular form. very few of them break apartand form ions in the solution. some of them do but theyonly partially ionized, that's the big difference between the strong acidsand the weak acids. ok. so everybody good? strong acids breakapart versus 100 percent
at the time, weak acids, don't. that's what you remember. it will serve you welljust to remember that. ok? this is that giveaway though, equilibrium. does everybody understand that? equilibrium, are you sure? ok, i'm going togive you an example that i think really goingto clear it up for you. we got all that?
>> how do we know if it'sgoing to be one equilibrium? like if we're given just thatfirst half side of the formula, how do we know that it'sgoing to back and forth. >> 'cause you're going toknow that's a weak acid because it's not on yourlist of strong acids. that's it. that's all, definitely yeah. that's all you know. >> so, you mean that's noton the strong list is going
to find the equilibrium. >> acids, yes. >> right. >> let me give you thisexample, as equilibrium because i think itwill really clarify it. clarify it not morethan it is right now. >> not all weak acids[inaudible]. >> it's always. >> yup.
>> ok. >> yup, they do because all weakacids have what we call a ka value which is equilibriumconstant. >> yeah, all right. >> let's get to look at this. this is just a little aside to help you understand morewhat equilibrium means. let's say that i have two tanks,two water tanks, all right? and my two watertanks are connected
at two points andthey have pumps. pumps only pump inone direction, let me try to get this, somewhat so i have two water tanks and iconnect it in two-- two points. and each of the pipes thatconnect them have pumps in them but the pumps are one way pumps. they can only pumpone way, right? and let's say i fillthis thing up. say i put-- better to maketoo high because i'm going
to add more water to it. say i have a hundred gallonsjust for the sake of argument. and i turn both pumps on, bothpumps, nothing's happening here with this pump becausethere's nothing in this tank, this tank is empty andi start pumping water between the tanksusing this pump. this is analogous to the initialstages of a reversible reaction. in the initial stages, only themore favorable reaction is going to be running, right?
because you have to generateenough product in order to initiate the reversereaction. so we're going to startpumping our water. so here's our water, right? and what's going to happen overhere is this is going to start to fill up, our forwardreaction, are more favorable, see which way they're going. this fills up and only one ofthe reactions is proceeding. until you hit a threshold value
where you initiate the reversereaction and water begins to be pumped backinto tank number one but it's still not being pumped in at the same rate that's evenpumped out, diameter in length of these pipes arethe same pumping power of the pump are the same. ok? so a little bit of thereverse reaction has started because you have to generatea threshold amount of product. the minute you form product, itdoesn't just immediately reverse
and go back, otherwise, you'd never see anyproduct form, right? not of it would ever be therebecause as soon as it form, it will immediately revertback to the reactants, to the reverse pathway. so you have to havea threshold amount of products before thereverse reaction to initiate. and this thing will keep going. once you hit a certainproduct or amount of product,
your rate of reverse isequal to your rate of forward and you have achievedequilibrium. remember equilibrium isabout rate, not amount. does the amount of water ineach tank have to be equal? no, it doesn't have to be. can it be? yeah, it can be butit doesn't have to be. all right, let's say forthe sake of argument, we started out with a 150gallons here and we ended
up with 50 gallons here, right? that means we pump 50 gallons out so this is nowat equilibrium 100. the amount of reactantsat amount of product at equilibrium donot have to be equal. equilibrium has nothingto do with amount. it has anything todo with rates. this looks like steady state. if you were up here in achair, looking down, you'd say,
"that tank is not movingand that tank is not moving. i'm in equilibrium. that looks like it'sa steady state. but in reality if youthrew a piece of there, you see the paper get suckthrough, come back up, get suck through, it's dynamic,there's process going on. this is moving. it's in equilibrium. it just so happens that therate of water being pumped
out of one tank is exactlythe same as the rate of water being pumpedinto the tank so it looks like nothing is happening,this is equilibrium. ok? the amount donot have to be equal. they can be but theydon't have to be. that's not a requirementfor equilibrium. what is interestingis that sense of-- it looks like steady stateand nothing is going on, the ratio of theamount of water needs
to take is a constantat equilibrium. in other words, let'ssay we want to take the ratioof this over this-- two, that ratio isconstant at equilibrium at specific temperature,it doesn't change. let's say we dump in 75gallons of water, what's going to happen, we'restressing this equilibrium. we put pressure on. here it is, nice and--everything is good,
100 gallons 50, and all of asudden, i dump a bunch of water and that thing is goingto go like this isn't it? and it's going to reestablish, it's good the chatelier'sprinciple, you'll learn it later. you stress the systemat equilibrium, it moves to relive thestress and reestablish, so we put 75 gallonsof water in here, this thing will reestablishat 150 and 75.
still equals to two. tthe ratio stays the same. this is equilibrium. this is what's going on whenyou ionize weak acids, partial. this is what's' goingon any equilibrium. and that ratio is aquantitative number. it's called equilibriumconstant, all right? you won't have aquestion on the exam. ok? in fact this is way morethan we would want you to know
but i think it wasn't difficult,you know, to present it and i think you have abetter understanding now of what the equilibrium is. a lot of people and me included. i remember when i wastaking intro chemistry, general chemistry,i remember them. i wanted to say equilibrium, the amounts were equal that'swhat it meant, you know, equilibrium, it's rightthere, it's in that.
ok, so we're going to memorizeour list of strong acids knowing that the strong acids donot obtain equilibrium. anything else that's an acid isnot on the list is a weak acid and they are in equilibriumwith their ions, ok? although the amount ofion production is very, very small, very small. ok? ok. so, we know thatacids produce h plus, and we know that basis have acouple of different definitions. we're going to probably going
to lean more toward theproton acceptor definition under bronsted-lowry but we'realways going to keep back in the back of our mind if wesee oh, we know that according to arrhenius, that is a base and that can help identify ourconjugate asset base pairs. so how do we quantitate, thehydrogen ion concentration? how do we put a number onit because we can do that, it's called the ph, ph. and incidentally the lowercasep doesn't mean anything.
i've seen some books and heardsome people say, oh it's power of hydrogen, or it'ssomething like that. it doesn't stand for anything. in fact, it just tellsyou that you have to do a mathematical operation. the ph is directly relatedto the molar concentration of h plus in a solution, ok? and it's a log function. the ph is equal to the negativelog of h plus concentration.
in fact h plus weactually mean h3l, right? but again, sometimes forconvenience, we say h, h, ph is much better than ph3l, ok? i hope everybody hastheir calculators, right? everybody got their calculators. i want you to locatethe log key, it's l-o-g. if you don't see it on the keyitself, look at the inverse of the 10 to the x cube. look in the blue for theinverse function on 10
to the x 'cause these areinverse functions of each other. does everybody see the l-o-g? yeah, big capitalletters, jumps out of you. ok? i love this calculations because they're prettymuch idiot proof. you can't take the logof a negative number. in other words, you can'ttake the log of negative two, it will give you an error, but you can take thenegative log of a number.
you just take the logof it, change sign. ok? so you don't have toworry about messing that up. if you try to take thelog of a negative number, your calculator isgoing to say, error. it means no are-- all right? something like that. ok? you'll be given theh plus concentration. all you have to do isdo the calculation. let's try it.
again these are brackets,these brackets, is very common in chemistry, meaningmolar concentration. that mean molar concentration,that's what those brackets mean. so molarity is whatyou're looking for. let' say, 2.1 times 10to the negative 4 molar. you can see what the ph is. now, some of you willhave to put the number in first then hit log, otherswill have to hit log first. and the easiest way to figure
out which one you are ishit the log key right now. if you see it spellslog in our screen, then you push the logkey then with the number. you could actuallyhit negative first. that works. you can actually hitthe negative, not minus, it will change sign key whichusually looks like this or this, you can hit the changesign key then hit log. mmm, i'll get to that.
how did you make thatcome out to three? can you set your calculator to show certain numbersin a contingent? >> no. >> good. because if you could,i want one of those calculators. >> i know, [inaudible]. >> ok. so, we're goingto put in our formula, ph equals the negative logof h plus concentration. i have the concentration--
what was that 3.-- >> 677-- >> 6 what? >> anyway, it's a 3.67 and a 8. >> yeah, give me-- giveme a couple of them. >> ok, here. >> 3 point. >> 677. >> 67.
>> 7. >> 80. >> ok, that's good. everybody get that? who did not get that? >> well, actually, actually 7. >> 77. >> 77780. >> 3.77780.
>> ok, who gave that? like that? ok. everybody got that right? but it's really a straightforward calculation, right? these are gimme points. easy to get points on the examso you can't afford to miss it. you can't afford it. so you make sure and dothese calculations correctly, all right?
now when you're taking the log, significant digitsare little different than what we're used to. how many significantdigit is in this number? >> two. >> two because it's writtenin exponential and we donate so that you can do it,like specific, right? we just say, it's writtenin scientific notation, count them all up, two.
when you take logs, whenyou hit the log key for phs, significant digits don'tstart until after the decimal. so two significant digits inthis number is right there. this answer is 3.68on the ph, ok? logs have two parts,to send an ordinance, and the significantdigits it's-- are related to one of those. we don't really care. let's just know thatit doesn't start
until after the decimal point. so you look at phs,10.41, 6.21, 0.51, this all have twosignificant digits. they're all two sig figs. be careful. be careful when you'redoing them. this is only for log. you only have to worry aboutit when you see ph equals. that's the only time you haveto worry about, other than that,
everything else is the same. ok? what it could,always remember that. ph is when you got, everylittle red light come on. now, the ph scaleruns-- 0 to 14. ph scale runs 0 to 14right at the middle is 7. right in the middle is 7. the acids are theless than 7 in ph. -- and the lower the phthe stronger the acid. so, these are the strongest.
these are weaker. that's kind of theopposite, right? you know, ph of 1 is astronger acid than a ph of 5. longer the ph, strongerthe acid. the bases run prettymuch the same. bases are up here,greater than 7 with the strongestbases of around 14. the higher the ph,the stronger the base. it's the opposite.
here's the weakerends-- weaker bases. again, 7. there's only oneneutral ph. and it's 7. 7 is the only neutral ph. ifyou'll 7.000000000000000, blah, blah, blah, 1 you are base. and if it's 6.9999999999 youget the drift, it's acid. 7 is the only neutral ph, ok? ok? what's the answer? >> it is a base, what's the ph?
>> it's 7.47. >> 7.47. it sounds about right. i got the red one. 7.47. >> yeah. >> 7.47, is over 7. it's in the basic range. ok. what's the ph? >> 7.00
>> 7.00, right? notice that this also could havebeen rewritten like of this. concentration of h plusis 10 to the negative 7. if you see somethingwritten like that, most calculators won't allowyou to just put in 10ee. i took or one, sorry. you don't want toput that in 10ee because that willactually put it off by a full other of magnitude.
you have to make it one,i understand negative 7. if you put it 10ee negative 7, its can actually make itone quarter bang to great. ok. that's would to kind of standing negative 7is what is ultimately. ok. ph is 7 makesthis neutral, right? so, you can tell kind ofqualitatively by looking at the exponent onthe base stand in the scientific notation.
negative 7 is your greyarea for neutrality. but if it's less thannegative 7, it's base. the last one we did was10 negative 8, right? negative 8 is lessthan negative 7. so, if it's less than negative7 you're looking at base. if it's greater than negative7 you're looking at an acid. i promise 100 percent you'regoing to have ph calculation on your quiz tomorrowand on the exam coming up for unit 3 through 6.
>> four through six? >> what? >> four through six. >> four through six,, sorry. four through six,. four through six. we just had three. >> sorry. if we write this andlook at this equation,
this is called self-ionizationof water. or the auto-ionizationof water, the same thing. and this happensanytime you have water. even aqueous solution, itdoesn't have to be pure water. anytime you have waterthis is going on. water is ionizing itself. if we go back to ourbronsted-lowry we say, we know this is anacid, this is the base. yeah. pick one, itdoesn't matter.
the self-ionization of water, notice in this case water canact as both an acid and a base. there are some compoundsor ions they can do that. they can act as an acidor a base depending on their local environment. these are called amphoteric. i've seen an amphiprotic,amphoteric. amphoteric that canadd as an acid. or base.
auto-ionization ofwater is an example of the amphotericnature of water. and water can act asan acid or a base. this is equilibrium andanything that's an equilibrium, it's most of the things, that are an equilibrium youcan calculate an equilibrium constant and you can dothat for this equation. we're not going to few them now. ok. we're not going tolook at the ratio product
to reactants at this point. but i will tell you that thereis in ion product constant. ion product times, right,multiply or times constant. and for water werefer to that is kw. this is the ion productconstant. it's only for water,that's why it's kw. the ion product constantfor water means that the concentration of h3oplus times the concentration of oh minus any solutioncontaining water is equal
to a constant, 1 times10 to the negative 14. ok. can you guys seethat in the back? barely. let me see if this one-- is that a little better? ok. what these allow us todo is calculate either one of this given the other one. so, if you're given thehydrogen ion concentration for a particular solution,you can calculate the ph. >> thank you.
or you can calculatethe oh minus. calculate the oh minus in a solution containingh plus 4.7 times 10 to the negative 4 mole. what do we got? >> 2.1 times 10 tothe negative 11. >> all right, yeah. 2.1 times 10 to the negative 11. that is correct.
all right? h3oh plus are thesame thing, right? divide it both sides. like 4.7 times 10 to negative 4. do them math, 2.1times 10 negative 11. molar. is this solution isacidic, basic or neutral? it's acidic. i got one acidic up here.
anybody second? >> yeah. pretty solid[inaudible] too. >> it's not bad, huh? >> is three or something. >> if the concentration-- if the concentration ofh3o is greater than 10 to the negative 7, youwill have a concentration of oh minus less then10 to the negative 7 because when you multiply
that together you haveto get a constant. so if 1 is-- pretend thenegative 7 is the break point, right? because that's neutral. the neutral solution says--can you see back here? you sure 'cause there'sseat right here. what is? do you wantto sit up here? >> no, it's fine. >> the neutral solution hasthe concentration of h3o equal
to the concentrationof oh minus. the only way you couldhave h3o equal to oh minus and when you multiply themyou get 10 to the negative 14. is it each one of themis 10 to negative 7? you can have h3oequal to oh minus 10 to the negative 3 molar,both of them, but guess what, when you multiply thoseconcentrations together you do not get the ion productconstant for water. so, in order to satisfy thetwo parameters, number one,
the concentrations areequal to each other and when you multiplythem together you get turn to negative 14. is-- if they're bothequal to 10 at negative 7? everybody see that. now, we did a problemearlier where i asked you to calculate the ph of eachsolution containing h plus equals 10 and negative 7 andthat ph came out to be 7.00. some of you may start to see.
there's no mistake here thatif you take the negative r of 1 times 7 negative14 you get 14, the upper amendmenton the ph scale. incidentally, you can't havea number outside, 0 and 14. so if you're on the examand it says calculate the ph and you get a number at 17? main mistake, wherewe can find it? you're answers can onlybe between 0 and 14. ok. so, this is theonly absolute situation.
if you get h3o plus greaterthan 10 of the negative 7, acid. if it's 10 to the negative7 then this is going to be definitely be lessthan 10 to the negative 7 because when youmultiply them together, you got to get 10 negative 14. and our base wouldbe the opposite. all you need is oneat them, right? given the concentration ofh3o or the concentration of oh minus you shouldbe able to tell
if it's an acid ora base or neutral. we're certainly mostfamiliar with h3o because that gives us ph.but there's an analogous to the scale called pohwhich is negative log of oh. we're all mess around with them. >> so let me ask asilly question probably but why is it negative11 and not negative 10? >> was it 10? >> no, i'm just asking howto get the negative 11?
>> i get it by dividingthis number by that number. oh, i see 'cause you're doingnegative 14 minus 4 is negative 10, right? >> because this numberis less than one. this is one-- i can see--let's say that it was four, ok. that'd be one-four, right. so, just for the sake of yourorigin, let's say that it was that and you want to do theshort hand method, you're going to say when i divide thatexponent i subtract that.
so, negative 14 minus anegative 4 is the same as negative 14 plus 4which means negative 10. and you're absolutelyright, 100 percent. here's the problem. what's 1 divided 4? what's-- >> point 25. >> point 25, is that anumber correctly written in scientific notation?
no it's not. you got to move thisover one which causes that to get smaller by one. so, whenever thenumbers don't come out to be exactly what they arelike if i'm multiplying i add, if i'm dividing isubtract exponents. whenever it doesn't come out tobe that number that means that, you know, your value in front of your scientific notationwas a number that's greater
than 10 or less than one. so, you got to move the decimal to make it a correctscientific notation. ok. everybody good? ok. you're going to have todo calculations involving kw and also calculationsinvolving ph, ok? i'm going to give you a littletable that's got a little bit more information than whatwe've covered in here. but i'm going to give it toyou anyway because somewhere
down the line i thinkyou're going to need it especiallyif take gen chem. and it relates ph, poh, h plus,the oh minus, all of this. ok, first i'm going to give youthe ones that we are using, ok. i'm going to draw arrowsand what this says is that if you have oh and youwant to go to h3o what you do-- -- is divide one 1times 10 negative 14 by the concentration of oh. and as you wouldexpect if you have h3o
and you want to go to oh minus-- -- you would divide it. this is kw, right? this is the kw calculations. whatever one you'regiven just divide it into the kw that's 1times 10 negative 14. divide it right into it,you can get the answer. if you have h3o andyou want ph-- you take the negativelog of the h3o.
so, when you're lookingat using this you're going to say what are givenversus what do i want? i'm giving h3o, iwant ph negative log. i'm giving h3o, i want oh, 1 times 10 negative 14divided what i was given. so, this is how it works. but there's no cheating. you can't cross. if you're given oh minus let'ssay we haven't done any of this
and you probably won't see it. but if you're givenoh minus and you want to know ph you followthe pathway. you start here. you first go to hereby doing that. once you get here yougo there by doing that. and really this is all we'reasking you to do, right? do calculations involvingph using negative log and calculate one giventhe other using the ion
for the constant. we don't ask you to come up withh3o given ph, but you can't. so, i'm going toput the ones in red that we're not necessarilyasking you to do. better make sure first. yes. we're just doingkws and ph. so, pretty much just stuff in black. but i'm going to fillin the rest for you in case you ever wanted to seeit or need it down the road,
because it's all pretty,pretty much straight forward. if we have h3o plusand we want ph, we take the negative log of h3o. if we have oh minus and we wantpoh, what do you think we do? negative log of oh, right? oops, this is got tobe in red now, right? i don't want you guys to beconfused with this stuff. negative log of oh. and so, that p whateverit is means negative log.
ph negative log of h pluspoh negative log of oh, pka negative log of ka,just stick to negative log. here are some ones thatyou might not have known. if you have poh andyou want to get the oh, you simply raise power of10 to the negative poh. so, if your poh is three and youwant to know what your oh is, it's 10 to the negative 3. you just raise 10 to thenegative power of the oh, the same thing over here
with ph. again you're notgoing to have to do this. if you have ph and you want to know what h plusconcentration is, you find your 10 to thex key in your calculator, you put in a negative phand you hit 10 to the x and it gives you the answer. lastly, we know that the phscale ranges from zero to 14. so, if you have ph and you wantpoh it's just 14 minus the ph, 14 minus the poh.
and you have yourselfa little table that relates allfour of the values. again, all we're goingto want you to do is run with kws and calculating phs. remember when youcalculate ph when you hit that log key remembersignificant digits don't start after the decimal. ok. this is all youneed to know, these three arrows for now.
if any of you go on university,take on chemistry, you're going to send me an emailsaying "oh, thanks." ok. questions? everybody good with thosecalcs, 'cause you're going to have quiz tomorrow, right? you're going to proveit to me tomorrow. we'll take the quiz beforewe start the lecture. ok, no, we can getout of the way. good? all right.
ok. we only got acouple more things. you can react acid with bases. this is a neutralizationreaction. an acid plus a base alwaysproduces a salt plus water, always. this is a general reaction type,acid plus base, salt plus water. this is nothing more than anydouble replacement, right? look at them. i'm going to put nawith cl and i'm going
to put h with oh, that's h2o. so, this is aquated. this is liquid. this is a subclass ofdouble replacement. which means all acid basereactions would be double replacement, but not all doublereplacements are acid bases. we've seen some doublereplacements. all of-- pretty much all oflab4 that's you're going to hand in today it's alldouble replacement.
it's called the neutralizationreaction. it's a neutralization reaction. we can write balancemolecular equations, balance formula equation right? ionic equations in thationic equations for this. let's pick a different one. there has to be. i don't want to use nacl, idon't have to and here's one. let's do the nitric acid.
i will do namingin just a minute. plus-- so we got that. nitric acid plussodium hydroxide goes to sodium nitrate and water. is it balance? looks balance to me. one sodium, one sodium,one nitrate, one nitrate, we really should be saying,one nitrogen, three oxygen, one oxygen, two hydrogen,were balance.
all right. total of four oxygen. three [inaudible]. do you recognize this is a salt? probably not, right? probably not. the most familiar saltto you is nacl, right? so, when i did this one up here, you probably, "ohyeah balances."
a salt is the anion of an acid. what's the anion of an acid? that's going to be anythingexcept the hydrogens that are written out front,that's the anion of an acid. so, is no3 the anion of an acid? of course it is. it's right there. that's on your listof strong acids. you'll get familiar with thoseanions once you start memorizing
the list of strong acids, and as you get exposeto other weak acids. ok. the anion of an acid-- -- combined with the cation-- -- other than hydrogen. of course it's otherthan hydrogen. if it was combined with hydrogenit would be the acid, right? as you become familiar with youracids this anions will become more and more familiar to you.
i just told you thatnitrate is the anion of an acid specificallythis acid right here. so, anytime you seenitrate was something other than hydrogen it's a salt. it's a salt. most ionic compounds-- i wantto say all ionic compounds but i hesitate to use that word,most ionic compounds are salts. they are anions of acids,whole bunch of acids combined with something otherthan hydrogen.
look at nacl. the anion is cl minus, thatis the conjugate base of hcl. remember that counting aspect. so, i don't want you toget stuck into thinking that nacl is the only salt. no, no, hundreds andhundreds and hundreds of salt. and most of them are solubleexcept for those specified and are solubility base. so, here's our balanceformula equation.
now we want to write ourtotal ionic equation. hno3 does that break apart? why? what is-- you want to say solubilityrules all nitrates are soluble? those applied to ionic compound,this isn't an ionic compound. what is this? >> polyatomic >> it is polyatomicbut what is h and no3?
what's the meaning of this unit? >> molecule, acid? >> acid. it's an acid, right? it's a strong acid, becauseit's on our list of strong acid. what do strong acids do? >> the salt break apart. >> break apart, virtually100 percent all the time. so, our solubilityrules are going to get kind of freakyon us here.
the solubility rules onlyapplied to ionic compounds. these were now talking aboutstrong acids and strong bases, weak acids and weak bases. strong acid, strong bases breakapart 100 percent all the time. weak acids and weak bases don't. hno3 is a strong acid. the only way i know thatis because i memorize it from the list of strong acids. and that's the only wayyou'll know it as well.
so, it does break apart. naoh separate apart. i know i haven't used[inaudible] changed your mind. naoh is a strong base. how do you know that? i'm not going to make youmemorize a list of strong bases. but if you look at your periodictable you can get a real good idea of strong basesbecause the hydroxide forms of these six started lithium,go down to the potassium
over to calcium,down the barium. that's a good start. otherwise, there'sa list of them. you showed me thatearlier, where is it? yeah. yeah. strong bases, we have startinghydroxide, potassium hydroxide and calcium hydroxide. i guess that's allwe could, you know. so, here potassium and calcium,so this-- just go these three.
they're right near each other onperiodic table group number one. you can't see? i know you can't see. ok. so, sodium hydroxidedoes break apart because it is a strong base. ok. an argument couldbe made, you know, using this solubility rules. i think something insolubility rule set, all hydroxide are insolubleexcept sodium, however,
it may have some exceptions. sodium nitrate, yup. this one now does applyin the solubility rules. it's a nitrate and sodium. so, we're going tobreak that apart. what about h2o, doesthat break apart? have we ever seenwater as an acid? yeah, we did, right? it can be a base too.
is it on our listof strong acids? and therefore it is a-- -- weak acid, right? and what we say aboutweak acids? they don't break apart. keep it together. all acid-base reaction, the driving force isthe formation of water. net-ionic--
cancel, cancel, cancel, cancel. we're left with-- there's our driving force. notice you can't see that. you wouldn't be ableto see the formation of water onto that, all right? you won't be able to seethat-- sorry, but it's there. any acid-base reactionsalt plus water-- these aren't handled anydifferently than the ones
that we saw previously with balance moleculartotal ionic and net ionic. ok? all right, let'sname these things. let's name our acids. acid nomenclatures, firstof all, all acids start with h. all acidsbegin with hydrogen. unfortunately, noteverything that begins with hydrogen is an acid. that's unfortunate part.
there are compounds that startwith h that are not acids. unfortunately, butfor us in naming all of our acids will start with h.the first thing we want to do-- -- identify the anionof the acid. we want to identify the anion. what is the anion? we just said thata minute ago right. this is everything-- -- except the hydrogen writtenout front or written first.
we just said that allacids start with hydrogen. in order to identify the anionall you have to do is cover up the hydrogens thatare written upfront. acid, anion. [ writing on boad ] here are some examplesor list of acids. what are the anion? everybody got thosewritten down? in order to determine what theanions are all you do is cover
up with the hs that arewritten out upfront. so, the anions clminus, so42 minus-- oh i put h3po4 for[inaudible] sake. we need to identify the anion. now, there's going tobe two main class sets. the first the aniondoes not contain oxygen. and then, the secondone we're going to do is the aniondoes contain oxygen. so, if the anion containsoxygen-- no, does not, right?
sorry. we're going todo-- does not first. the anion does notcontain oxygen. if the anion does notcontain oxygen you are going to name the acidhydro, root, ic acid. example, hbr. anion no oxygens. hydrobromic acid. if it doesn't have oxygenin it you will start with the prefix hydro.
hcn. what is it? what's cn minus? >> cyanide. >> cyanide right? so, it's got to behydro something, right? hydrocyanic acid. notice it's cyanide, bromide. so, i mean you couldmake an argument
that you change the ide to ic. this was bromide, becomesbromic, hydrobromic, ok. but the roots are, youknow, they're going to be pretty thesame as they were when we are doing inorganicnomenclature, binary compounds, chloro, bromo-- i'msorry, chloride, bromide. ok. now, what happens ifit does contain oxygen? if the anion does containoxygen, the first thing you have to do is name the anion.
if the anion containsoxygen you more than likely have a polyatomicion and whether you notice that are not most of yourpolyatomic ions end in ate or ite, nitrate, nitrite,phospate, phosphite, oxalate, i don't know what oxalate are. ok? name the anion. if the anion ends withate, drop the ate-- -- and add ic plusthe word acid. hno3, no3--
nitrate. nitric acid. hc2h3o2. what is the anion? c2h3o2 minus, what is that? acetate-- -- acidic acid. and it's highly purifiedform glacial acidic acid. this is vinegar,you might eat it. name the anion if theanion ends in ate drop ate
and add ic plus the word acid. there are two exceptionswhere the strict application of this doesn't give you thename of the acid except h2so4, so4 is sulphate, atedrop ic sulphic, no. this is sulfuric acid. the other is h3po4 which becomesphosphoric acid, not phospic. everything else is pretty good. everything else falls in line,pretty darn good with our rules. if the anion endswith ite drop the ite
and add ous plus the word acid. so, ates become ic,ites become ous, ates becomes ic,ites becomes ous. hno2, anion, no2minus, nitrite-- -- nitrous. we have the same exceptions. h2so3 becomes sulfurous. h3po3 becomes phosphorous. ok. you already memorizedyour polyatomic ions so,
this is just extracredit, right? this is just another exam whereyou get to give more points because you memorizethose polyatomic, right? anything that-- all acid startwith h once you have an acid, remember this is onlyfor acid naming, ok? it's not for anythingthat starts with an h. so, identifythe anion. if the anion does not containoxygen hydro, root, ic acid. if the anion does containoxygen you name the anion.
h becomes ic, ites become ous. this is acid naming. notice, you will neverhave hydro on an acid that has oxygen, right? hydro is reserved onlyfor anions with no oxygen. let's try one. let's try a couple,let's see, [inaudible]. do you have your list? i don't want to give youanything in anions [inaudible].
what is that? >> carbonic acid. co32 minus is carbonate. how did you know that? you memorize it. carbonic acid. >> chloric acid. >> chloric, yes, very good. clo3 minus is chlorate.
chloric acid. notice hcl, what's hcl? what's hcl? hydrochloric. notice how close they are. chloric acid versushydrochloric acid, only a name, formula is no, not at all. ok. so, you will see those the acid-base titration sectionwe're going to cover in lab.
we're going to performin the lab and doing the calculations so. there's nothing in the bookexcept for description, so read that over andjust be ready for lab. we're going to-- we'lldissect that pretty good. one of your practicalapplication of the titration. the last thing is buffer. buffer solutions. does anybody knowwhat a buffer is?
buffer, buffers are solutionsthat resist changes in ph. with small additions. buffers are solutionsthat don't change their ph when you add a little bit ofacid or a little bit of base. you can overload a buffer. you can add so much acid that itoverloads a buffer and you start to see the ph plummetbecause it's acid. the best buffers are weak acidsand their conjugate bases. the best buffers aremade up of weak acids
and their conjugate base. ie-- acidic acid, acetate. if your buffer resists changes,when you add small amounts of acid or base, does itmake sense that they have to have someway to neutralizethat added acid and added base? otherwise, that added acid oradded base would affect the ph and cause it to change. so, something in the bufferhas to be able to deal
with those added acid or baseand this is what it is, ok? if h3o plus is added, would youthink neutralizes the added h3o plus between this and this. what is h3o plus? >> h positive. >> h plus, yes, samething, right? what is it though? what's the name of this unit? it's an acid right?
remember you don'tsee it all the time but when you do it'salways an acid. so, which one of thesecomponents is going to neutralize that? the base. the base will, andthis is the base. remember these areconjugate acid base pairs. they only differby one hydrogen. this is the acid.
this is the base. so, if i add acid,it's neutralized by the basic component. alternatively we could show thatas h3o plus, plus c2h3o2 minus, we go to hc2h3o2 pluswater, same thing. just that shortcut wayyou take the water out. if oh minus is added whatcomponent neutralizes the added oh minus? the acid, right?
the acid, because oh is a base. so, here we would have theacid component reacting with the added base. now, this is a weak acid. this is not on ourlist of strong acid, which means it onlypartially ionizes. it only partiallygives up its h plus. ok? it doesn't wantto give up its h plus because it is a weak acid.
but faced with a strong basethat strong base will go in there and reapthat thing right off and it will haveanything to say about it. it won't give it up normally orvoluntarily but with the base and solution it sure theheck, come off, all right. so, this comes off and we get-- the oh grabs the protonand forms the acetate. now, we see how a buffer works. a buffer has both an acidic andbasic component, a weak acid
and its conjugate base. if you have a weak acid we know that weak acids don'twant to break apart. they only break apart partially. it partially ionized, right. so, the h plus the proton andthe anion are happy together. they don't want to break up. so, the base, theconjugate base is very strong because if you put an h plus inaround this acetate it's going
to grab it real quick and becomethat which is very [inaudible]. so, weak acids don'twant to give up protons, have very strong conjugate basesbecause the bases don't want to grab those protons and formthis thing back, all right? weak acids have strongconjugate bases. it's always the opposite. strong acids have weak bases. strong bases haveweak conjugate acids. it's always the opposite, right?
these two components,the weak acid and the conjugate baseare capable of dealing with any added acid orbase in the buffer solution and they neutralize itbefore it has an opportunity to affect the hydrogenion concentration, the ph. if you add acid,the base goes in to action. if you add base theacid goes into action. but notice what'sproduced in each reaction. if we had acid what's produced?
acid, right? if we add base what's produced? base. this is interesting, 'cause this is how thequestions are going to be asked. we're going to want to knowhow will a buffer respond to added acid or base? and i'm going to show the realeasy way to get those answers. we just said that if youadd acid the buffer response by producing its acid.
if you add base the bufferresponse by producing its base. so, once you know whatyour buffer looks like-- don't read into theseproblems, ok? don't read into them. don't make them more difficult. first of all you're goingto know what your buffer is. you're going to know theacid and the conjugate base. it's going to be given to you. so, you label it.
these are conjugateacid base pairs. which one is the acid? yeah, this is the acid,this is the base, right? what are we adding? >> base. the buffer responseby producing base, that. whatever you're addingacid or base, in this case we're adding base, go to your conjugate acid basepairs and identify your base. the buffer response byproducing more of that.
that makes sense, because theoh is going to be neutralized by this which you're goingto reap that hydrogen off and make that co3, 2 minus everybody understand that? and the answer willbe by producing more. ok, those will be the answer. and it doesn't matterwhat it looks like. how will this bufferrespond to added h plus? [ inaudible response ]
which is? >> the h2-- phosphate. >> that's right. >> or the dihydrogen-- >> dihydrogen phosphate. notice you wouldn't useacid naming on this, right, 'cause it's not an acid. acids are neutral. our naming was onlyfor neutral acids.
this is a polyatomicion which you memorize. if it's neutral, we can usethe procedure we just developed for naming acids. if it's not neutral andthere's got a charge on it, it's got to be one polyatomicions, so you remember those. this buffer wouldrespond by producing-- ok? i'll do one more. that's actually astrong acid, right? i don't want to use the strongacid, 'cause it's not right.
sorry guys. we need to pair [inaudible]. yeah, let's-- how--this content-- added oh. oh, how that respond? more base which is-- which one? here is our acid. there is our base. questions?
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