You have two 500.0-mL aqueous solutions. Solution Ais a solution of a metal nitrate that is 8.246% nitrogenby mass. The ionic compound in solution B consists ofpotassium, chromium, and oxygen; chromium has anoxidation state of +6, and there are 2 potassiums and1 chromium in the formula. The masses of the solutes ineach of the solutions are the same. When the solutionsare added together, a blood-red precipitate forms. Afterthe reaction has gone to completion, you dry the solidand find that it has a mass of 331.8 g.
a. Identify the ionic compounds in solution A andsolution B.
b. Identify the blood-red precipitate.
c. Calculate the concentration (molarity) of all ions inthe original solutions.
d. Calculate the concentration (molarity) of all ions inthe final solution.
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Chemical Principles
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