Question #44683

This question tests the intersection of electrochemistry and intensive solution properties.

The primary trap is the 'Limiting Reagent' oversight: students often blindly apply Faraday's Law ($m = \frac{MIt}{nF}$) to calculate the theoretical yield ($388.8 \text{ g}$) without verifying if the solution contains enough electrolyte.

The secondary trap is the 'Density Assumption': students frequently assume the density of an aqueous solution is $1 \text{ g/mL}$ or equate the solution volume to the solvent mass, which drastically alters the calculated moles of \ce{Ag+} (yielding $216.0 \text{ g}$).

By using a highly concentrated saturated solution, the textbook assumption of $d \approx 1 \text{ g/mL}$ is invalidated, forcing a rigorous derivation of mass fraction.