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(a) Referring to Figure $16.6,$ describe how you would determine the $\mathrm{p} K_{\mathrm{b}}$ of the base. (b) Derive an analogous Henderson-Hasselbalch equation relating pOH to $p K_{b}$ of a weak base $B$ and its conjugate acid $\mathrm{HB}^{+}$. Sketch a titration curve showing the variation of the pOH of the base solution versus the volume of a strong acid added from a buret. Describe how you would determine the $\mathrm{p} K_{\mathrm{b}}$ from this curve. (Hint: $\left.\mathrm{p} K_{\mathrm{b}}=-\log K_{\mathrm{b}} .\right)$

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a. $\mathrm{p} K_{\mathrm{b}}=\mathrm{pOH}-\log \frac{[\text { conjugate acid }]}{[\text { base }]}$b. $\mathrm{p} K_{\mathrm{b}}=-\log K_{\mathrm{b}}$

Chemistry 102

Chapter 16

Acid-Base Equilibria and Solubility Equilibria

Acid-Base Equilibria

Aqueous Equilibria

University of Central Florida

Drexel University

University of Kentucky

Lectures

00:41

In chemistry, an ion is an atom or molecule that has a non-zero net electric charge. The name was coined by John Dalton for ions in 1808, and later expanded to include molecules in 1834.

24:14

In chemistry, a buffer is a solution that resists changes in pH. Buffers are used to maintain a stable pH in a solution. Buffers are solutions of a weak acid and its conjugate base or a weak base and its conjugate acid, usually in the form of a salt of the conjugate base or acid. Buffers have the property that a small change in the amount of strong acid or strong base added to them results in a much larger change in pH. The resistance of a buffer solution to pH change is due to the fact that the process of adding acid or base to the solution is slow compared to the rate at which the pH changes. In addition to this buffering action, the inclusion of the conjugate base or acid also slows the process of pH change by the mechanism of the Henderson–Hasselbalch equation. Buffers are most commonly found in aqueous solutions.

03:47

Sketch the titration curve…

02:05

Sketch the titration cur…

05:55

Consider the curve shown h…

01:53

02:33

Hello. Said that I was going to be talking about how we confined the PKB off. Ah, weak base. So consider this Thai tradition curve where we have ah, weak base. We're adding strong acid, hydrochloric acid. And we get this tight Trey shin curve. So how couldn't we find the PKB? Well, remember that this will be the equivalents point where all of the we're all of the bass has been converted toe acid. So halfway to the equivalents point half of the base will be converted to the contract acid. So that means if you remember the Henderson Hasselbach equation that this pot right here with the pH will equal the peak a of the country get acid. And if you remember, you know that Okay, Times the K B is equal to K W. Takes a lot of good log of everything. So the PK plus the PKB is equal to the P K W, which is 14. So the PK plus the PKB is equal to 14. Now we can find the peak a because at this point, half of the base will be converted to the conjugal acid. So if you know the PK of the conjugal acid. We can find the PKB off the what of the base that we started off with now? So we know that the Henderson Hasselbach equation is the pH is equal to the peak. A plus the contract base over the lot, plus the log of the country gave base over the acid. But what about we try to write this in terms of the p O. H. So with the P O. H, we have a base that's reacting with water to give the conjuring acid and hydroxide. So the PKB well, the K B is equal to the acid. Change the hydroxide over the base. So now let's rearrange this can have High Doc set in the side. Then we're going to have K B Times base over the conjugal acid. So now let's take the negative log of anything of everything's with the negative. Log. Hydroxide is equal to the negative log of K B. My nest log. It's the base over the country. Get acid. So the negative Aga for hydroxide assist appeal age. The negative log of the K B is just a PKB, and then let's make this a positive log. I won't do the conjugate acid over the concentration of the base. So there we go. And this is analogous to the pH here. So if we draw Thai tradition curve where instills of pH, we have the P o. H. And then we have the volume of hydrochloric acid. Instead of starting off on high Pete Ph like we did here, it'll be a low p o. H. Because there is quite a bit of hydroxide because this solution is basic, then will end up with an acidic solution with a low P o. H. And so here will be the 25 the volume we need to get to equilibrium, toe to the equivalence point and then half of that. And but at half way to the equivalents point, we will see the pH is equal to the Pekka at P. O h. Wait. I mean, the P. O. H. Is equal to the PKB. As you can see up here when this log will be zero and then the p o h will simply you called it PKB

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