1. The problem statement, all variables and given/known data I have to calculate the KSP of Ag2CRo4. I did this lab several days ago and I'm completely stumped. If anyone could help me out here, at the least guide me in the right direction so I can get this done as I am getting very frustrated :P Here is the data I have derived thus far. 2.5x10-5 = concentration of AgNO3 1.5x10-5 = concentration of K2CrO4 Using a concentration / absorbance chart, we found the conc. of the CrO4-2 ion, 1.24x10-3. My teacher says that the concentration of the Ag+ ion can be found stiochiometrically by using the CrO4-2 ion, then we can calculate KSP from that. I have no idea of how to get to the concentration of the Ag+ ion though. The instructions say this: 1. "Determine the value of Q for your original mixture of 5.0 mL of 0.0050 M AgNO3 mixed with 5.0 mL 0.0030 M K2CrO4. Keeping in mind that a precipitate forms from this mixture, is the actual Ksp for Ag2CrO4 greater or less than this value?" the diluted concentrations of those molecules are listed above. 2. Perform necessary calculations in order to determine the Ksp for Ag2CrO4. This would include: a. calculation of chromate ion concentration using the equation of your line from day 1. b. Calculation of the silver ion concentration. c. Calculation of Ksp for Ag2CrO4." The chromate ion concentration is 1.24x10-3. 2. Relevant equations AgNO3 + K2CRO4 <-> Ag2CrO4 + KNO3 Ag2CrO4 <-> 2Ag+ + CrO4-2 Ksp = [Ag+][CrO4-2] All are aqueous, except Ag2CrO4 is solid. I don't really have an "attempted solution" for this exact calculation because I really don't know what to do next. I've been able to calculate all of the necessary ingredients up until now. Thanks in advance for anyone who is willing to give me some guidance / show some calculations.