Chapter 15, Problem 77AE

A solution contains 0.018 mole each of I⁻, Br⁻, and Cl⁻. When the solution is mixed with 200. mL of 0.24 M AgNO₃, what mass of AgCl(s) precipitates out, and what is [Ag⁺]? Assume no volume change.

$\begin{array}{l}\text{AgI:}{K}_{\text{sp}}=1.5\times {10}^{-16}\\ \text{AgBr:}{K}_{\text{sp}}=5.0\times {10}^{-13}\\ \text{AgCl:}{K}_{\text{sp}}=1.6\times {10}^{-10}\end{array}$