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Considering the results of the addition of acid or base to abuffered solution and contrasting those to the results when acid orbase are added to unbuffered water, b...

Question

Considering the results of the addition of acid or base to abuffered solution and contrasting those to the results when acid orbase are added to unbuffered water, briefly discuss theeffectiveness of buffers in resisting pH changes.

Considering the results of the addition of acid or base to a buffered solution and contrasting those to the results when acid or base are added to unbuffered water, briefly discuss the effectiveness of buffers in resisting pH changes.



Answers

Compare the results of two experiments: First, a small amount of base is added
to an unbuffered solution with a pH of $7 .$ Second, the same amount of base is
added to a buffered solution with a pH of $7 .$

So we want to know the effect of adding a small amount of a strong acid or base, usually too a buffer. And basically the answer is that the effect will be a small change in the pH. It's not true that above her prevents the change in pH. It resist, sit and makes it small. So, for example, if you added some HCL to water, the pH might go Ah, from 7 to 4 from 7.2 uh, 4.0. Ah, And if you add it to the same amount of HCL was added to a buffer, then the pH, if you had a buffer at Ph. Seven to Ph, might go from seven to 6.9. So it's not no change. It's a small change in the pH and really the effect on the buffer. If you have a buffer of, say, so you're adding some age seal to a buffer contains the hypochlorite I on and Hypo course acid. Well, if you add a little bit of ah, hydrochloric acid, uh, almost all of it will react with the O. C. O minus. And so it's concentration will decrease, and almost all of that age plus that you added Ah by reacting with e o C L minus. Uh, the OOCL minus will be converted to, uh, hcl. Oh, and so you get a change in the concentrations of the substances in the buffer. But nearly all of the strong acid that added is consumed, and so you just get a small change in the ph.

This question is in reference to how a buffer solution works. If you add a strong acid to water, there is a significant decrease in ph but adding a strong acid to a buffer solution does not appreciably decrease the ph when adding a strong acid to water, Every single mole of strong acid reacts with water producing hydro Nehemiah on. Therefore we get a significant increase in the hydro Nehemiah and concentration with the increase of a strong acid to water. However, if we add a strong acid to a buffer, a buffer is a buffer because it contains a weak acid and its conjugate base, therefore it contains an acid and a base. So the addition of a strong acid to a buffer solution will allow the base of the buffer system to react and neutralize the incoming strong acid. So adding a strong acid to the buffer, the hydro knee um from the strong acid reacts with a weak base of the buffer, forming the conjugate acid of the week base or forming more of something that's already in the buffer system. Thus we are decreasing the amount of hydro Nehemiah that is incoming from the strong acid. Yes, we are decreasing the amount of hydro Nehemiah on that is being added. Then we are decreasing the change in ph so the ph would not drop near as much when added to a buffer system versus adding it to water. Here's a picture showing that the addition of hcl, which is the addition of H 30 plus allows the H 30 plus to react with the X minus which is the base that is present, forming a checks which is already in solution and water.

I'm doing a voice over on this one. So in this problem were given acetic acid ch three C O h, which is a weak acid and N h. And were asked. We're told that mixing together solutions of citric acid and sodium hydroxide can make a buffered solution. And how does this happen? How does the amount of each solution added change how effective the buffer is? So here's what happens when we combine the city gas it and the There's the acetate ion Plus I had drawn in my aunt plus the sodium ion. I can't believe I didn't put charges on those. There's a book. There we go. So there's my charges and we have a no a giant. And look what those two dio those two together. What happened there? Those two together, the H 30 plus and the minus. There's weak acid strong base, so the sodium acetate is going to create my salt, and that's going to be my weak acid and its assault. The sodium acetate will be my weeks, my my assault of my weak acid. So if I increase the concentration of the weak acid, I'm going to shift to the right and increase the concentration of the asked ion. This is the second part of the the questions, The question said. How would adding either one of the reactions change the concentrations or change the effectiveness of the buffer? So if I add more weak acid, I'll shift to the right and that will make us amore effective buffer because I have a greater amount of myself. If we add more sodium hydroxide, I'll have a greater amount of sodium and hydroxide ions. So once I have more hydroxide ions is going to reduce my effectiveness because once I have more hydroxide ions, we will shift to the will shift to the left. I think I have another question here. How would you would have buffered solution made by HCL in N a. O. H. Be affected? No, it would not, because that's a strong acid and a strong base. And they do not form buffer solutions because there's complete dissociation of each of the acid and the base, and that should be it for this problem. The hell is a completely dissociated salt. Okay, I'm done


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