## Problem 6.63

Matt Sanruk 2H
Posts: 131
Joined: Wed Sep 18, 2019 12:21 am

### Problem 6.63

How did you guys approach this problem and how can you get the pH from voltage and vice versa?

Sebastian Lee 1L
Posts: 157
Joined: Fri Aug 09, 2019 12:15 am
Been upvoted: 1 time

### Re: Problem 6.63

When working with a pH electrode meter you have the following equation: $E=E^{\circ}-\frac{RT}{F}ln[H^{+}]$.
This is derived from the Nernst equation where in this case, Q is just the concentration of H+ because in buffers, [HA] and [A-] are the same.

From here, you know that you are given the cell potential (E cell) at a certain pH. We can turn pH into [H+] and then solve for $E^{\circ}$ of the reaction because we know what the E cell for that H+ concentration is. From here, you can use that same equation to solve for the unknown [H+] because you are given E cell and you've just found E naught. Then you would find pH from the [H+].

Matt Sanruk 2H
Posts: 131
Joined: Wed Sep 18, 2019 12:21 am

### Re: Problem 6.63

Oh I see this equation would make this a lot easier to solve. Thanks!