AgNO3 is slowly added to a solution containing 0.010 M Na2CrO4 and 0.050 M KBr. Given: Ksp(Ag2CrO4) = 1.1 × 1O−12 ; Ksp(AgBr) = 5.0 × 1O−13 . 3.1 Show all your calculations and reasoning to prove that AgBr will precipitate first. 3.2 What is the percentage of Br− that remains in solution at the instant when the precipitation of Ag2CrO4 starts? 3.3 How would the solubility of the AgCrO4 be affected, if a few drops of ammonium chromate is first added to the solution containing the salts (before adding any AgNO3 ?) You must only write "increase" or "decrease" or "stay the same" and briefly explain your answer in one sentence.