1. The problem statement, all variables and given/known data What is the minimum quantity of ammonia which must be added to 1L of a solution in order to dissolve 0.1 mole silver chloride by forming [Ag(NH3)2]+. Given Ksp- 10^-10 and Kf- 10^8 2. Relevant equations 3. The attempt at a solution I used the equation (which I derived) s=c^2/(Ksp)(Kf) (assuming almost all amount of AgCl converts to complex and some other approximations) where s is the solubility of AgCl and c is the concentration of NH3 (both in mol/litre) I solved and got c as 1 mole. But answer given is 1.2 mole. Are my assumptions wrong, or there is some other thing?