1. The problem statement, all variables and given/known data Hi, I need to calculate the Ksp of Ag2CrO4 based on experimental data. During the experiment, 1.25g of pure copper was placed in a 1.00 L solution of silver chromate. When the copper was extracted, only 1.24g remained. Balanced chemical equation: Cu + Ag2CrO4 --> CuCrO4 + 2Ag 3. The attempt at a solution Here's what I did: mole of copper = 0.01g / 63.546 = 1.57 * 10^-4 Since volume is 1.00 L, the number of moles is equal to the concentration. There are 2 moles of Ag and 1 mole of CrO4 for every mole of copper, so: Ksp = (1.57 * 10^-4) (3.15 * 10^-4) (3.15 * 10^-4) = 1.56 * 10^-11 But this doesn't seem correct because the actual value is 1.1 * 10^-12. This would give me a percentage error of over 1000%... Any help would be much appreciated.