Chemistry, 11.10.2019 03:50 paigejohnson955
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 two potassiums and 1 chromium in the formula. the masses of the solutes in each 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 it has a mass of 331.8 g. identify the ionic compounds in solution a and solution
b. identify the blood-red precipitate. calculate the concentration (molarity) of all ions in the original solutions. calculate the concentration (molarity) of all ions in the final solution.
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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%...
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