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Determining Concentration from Cell Potentials

CHEM-FQVLRJ

Consider a galvanic cell at $25 °\textrm{C}$ based on the unbalanced reaction below.

$$\textrm{MnO}_{4(aq)}^-+ \textrm{H}^+_{(aq)}+ \textrm{Fe}_{(s)}\rightarrow \textrm{Fe}^{2+}_{(aq)}+ \textrm{Mn}^{2+}_{(aq)}+ \textrm{H}_2\textrm{O}_{(l)}$$

Given $\left[\textrm{MnO}_4^-\right]=0.600 \textrm{ M}$, $\left[\textrm{Fe}^{2+}\right]=0.150\textrm{ M}$, $\left[\textrm{Mn}^{2+}\right]=0.0100\textrm{ M}$, and the $\textrm{Fe}$ electrode has a mass of $20.0\textrm{ g}$, determine the pH in the cathodic compartment if the cell potential is $1.740\textrm{ V}$.

Use the table below to find the standard reduction potentials.

What is the pH in the cathodic compartment?

A

2.44

B

2.70

C

5.03

D

5.41

E

6.20