Question #44750

Two electrolytic cells, X and Y, are connected in series. Cell X contains $500\text{ mL}$ of $0.30\text{ M } \ce{Ce(SO4)2}$ in dilute $\ce{H2SO4}$, and Cell Y contains an aqueous solution of $\ce{CuSO4}$. A constant current is passed through the cells until $1.5875\text{ g}$ of $\ce{Cu}$ is deposited at the cathode of Cell Y. The electrolysis is then stopped. The resulting solution from Cell X is completely titrated with $0.10\text{ M } \ce{FeSO4}$ solution. What is the volume of $\ce{FeSO4}$ solution required to reach the equivalence point?\n\n(Given: Atomic mass of $\ce{Cu} = 63.5\text{ g/mol}$, $E^\circ_{\ce{Ce^{4+}/Ce^{3+}}} = +1.61\text{ V}$, $E^\circ_{\ce{Ce^{3+}/Ce}} = -2.34\text{ V}$, $E^\circ_{\ce{H+/H2}} = 0.00\text{ V}$)