1. The problem statement, all variables and given/known data What percentage of the original Ag+ remains in solution when 175 mL of 0.0208 M AgNO3 is added to 250 mL 0.0380 M K2CrO4? 2. Relevant equations 3. The attempt at a solution I found the initial amont of CrO4 and Ag and put that into the equilbrium expression of AgCrO4(s). I let the reation complete and used Ksp for the back reation to find the ions in solution. but i couldnt get the right answer. Question 2: If 100.0 mL of a clear saturated solution of Ag2SO4 is added to 266 mL of a clear saturated solution of PbCrO4 how much precipitate in mg will form? For this problem, ignore the back reaction since it will have an insignificant effect on the amount of precipitate that forms. The molecular weight of PbSO4 is 303.26 g/mol and the molecular weight of Ag2CrO4 is 331.73 g/mol. Give your answer to three significant figures. Attempt to the question So I tried finding the concentration in PbSO4 and Ag2CrO4 using Ksp expression. and used to concentration to find moles. used moles and molar weight given to find the weight. and I added the two up. And again I got an incorrect answer.