Ch 14 Exercise 43

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

Ariana_Kermani_2G
Posts: 10
Joined: Fri Jul 15, 2016 3:00 am

Ch 14 Exercise 43

A tin electrode in 0.015M Sn(NO3)2 (aq) is connected to a hydrogen electrode in which the pressure of H2 is 1.0 bar. If the cell potential is 0.061 V at 25 degrees Celsius, what is the pH of the electrolyte at the hydrogen electrode?

Which equation are we supposed to use to solve this problem?

Thanks!

Arshia_Sabir_3E
Posts: 13
Joined: Wed Sep 21, 2016 2:59 pm

Re: Ch 14 Exercise 43

Use the Nernst equation in order to calculate the PH of the electrolyte at the hydrogen electrode.
You can start with E=E(node)-(0.0256V/n) ln([Sn^2]/[H^+]^2) and Just solve for the concentration of [H^+]^2.
Then convert that concentration to PH by -log([H^+]

Hope this helps!

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