please help i am having a hard time getting this. Step by step please much appreciated.

2. You have two 500.0mL solutions. Solution A is a solution of a metal nitrate that is 8.246%N by mass. The ionic compound in solution B consists of potassium, chromium and oxygen. Chromium has an oxidation state of +6 and there are 2 potassiums and 1 chromium in the formula. The masses of the solutes in each of the solution are the same. When the solutions are added together, a blood red precipitate forms. After the reaction has gone to completion, you dry the solid and find that is has a mass of 331.8g. a. Identify the ionic compounds in solution A and Solution B. b. Identify the blood-red precipitate. c. Calculate the concentration (molarity) of all ions in the original solution. d. Calculate the concentration (molarity) of all ions in the final 500mL solution