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# In the reaction barium chloride plus potassium chromate

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In the reaction barium chloride plus potassium chromate yields potassium chloride and barium chromate, 10.0 milligrams of barium chloride is mixed with 1.00 grams of water to make a barium chloride solution, which has a volume of exactly 1.00 ml. It is titrated with a solution of 100 grams of potassium chromate dissolved in sufficient water to make 5000 ml of solution. Calculate the following:

1. The mass percent of the barium chloride
2. The molarity of the potassium chromate solution
3. The volume of potassium chromate solution required to react with all the barium chloride solution
4. The mass of potassium chromate required to react with ten times the volume of the barium chloride solution
5. If 100 grams of barium chloride were dissolved in sufficient water to make 1 liter, how many grams of potassium chromate would be required to react completely with all the barium chloride?

https://brainmass.com/chemistry/stoichiometry/61590

#### Solution Preview

First write the balanced reaction:
BaCl2 + K2CrO4 = 2KCl + BaCrO4

1. Mass percent of BaCl2
10mg=0.01(g)
Mass % of BaCl2=mass of BaCl2*100/Total mass=0.01*100/1.01=0.99(% w/w)

2. The molarity of the potassium chromate solution
Molecular weight of ...

#### Solution Summary

The solution provides detailed explanations and calculations for the problem.

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