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You have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246% nitrogen 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 solutions 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 it has a mass of 331.8 g.
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 solutions.
d. Calculate the concentration (molarity) of all ions in the final solution.
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