1. The problem statement, all variables and given/known data What mass of AgCl will dissolve in 1 L of water containing 0.0144 moles of NaCl. Ksp = 1.7 x 10^-10 2. Relevant equations Ksp = [x][x] and ICE table 3. The attempt at a solution So, the common ion effect is taking place here and the equilibrium taking place is: AgCl(s) ↔ Ag+ + Cl- Since excess Cl- will be present from the NaCl, the Na+ is just a spectator ion. ICE table: AgCl(s) ↔ Ag+ + Cl- x 0 0.0144 M -x x x 0 x 0.0144 + x Ksp = [Ag+][Cl-] = 1.7 x 10^-10 (x)(0.0144 + x) = 1.7 x 10^-10 I assume that I can eliminate the x in the parentheses because it would be very small, thus: 0.0144x = 1.7 x 10^-10 x = 1.2 x 10^-8 mol/L Converting to grams gives me 1.8 x 10^-6 g/L I was wondering if someone wouldn't mind checking to see if my steps are accurate. Thanks in advance!