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# Stoichiometry

## Repetition exercises

1.Calculate the molar mass of the barium hydrogensulfate.

2.Calculate the mass of 3.5 moles of sulfuric acid.

3.How many moles of hydrochloric acid are in 3kg 5% acid?

4.A solution of nitric acid at 12.33% has a specific mass of 1.070 g/cm 3. Calculate the mass of 3 L of this solution and then the number of moles of nitric acid therein.

5.Calculate the mass of one liter of a solution of sulfuric acid to 98.52% (density of this solution = 1.8405), then the number of moles that are in a liter (called molarity)

6.A solution containing 1.465 g/cm3 of sulfuric acid has a specific mass of 1.765 g/cm3. Calculate the mass of one liter of the solution, then the content percentage of the acid in one liter of this solution.

7.A 4.84 molar solution (containing 4.84 moles per liter) of hydrochloric acid has a density of 1.065. Calculate the volume of 100 g of solution, then the mass of acid therein. (Thus we calculated the percentage of acid in this solution)

8.A 10% solution of perchloric acid has a density of 1.0597. Calculate the molarity of the solution (molarity = number of moles per liter).

9.Calculate the percentage (mass in 100 g) of iodine in a solution of hydroiodic acid, specific mass 1.0751 g/cm3 and molarity equal to 0.841 mol/L.

10 What mass of barium sulfate can be precipitated from 10 g of a solution of 5% barium hydroxide and an excess of sulfuric acid?

11. Calculate the mass of calcium hydroxide which can be obtained from 40 g of quicklime (calcium oxide) and then calculate what volume must have a 0.01 molar solution (moles per liter) of this hydroxide.

12. Sodium is burned in the air and the oxide obtained is introduced into water. What mass of sodium did one burn, if finally one has 2 L of a 0.2 molar sodium hydroxide solution?

13. What volume of 0.1 molar solution of silver nitrate was used to form 2 g of precipitate by adding an excess of solution of sodium chloride salt?

14. From 100 ml of a solution of potassium carbonate, there were obtained 3 liters of carbon dioxide under standard conditions. Calculate the molarity of the solution of potassium carbonate and the mass of potassium carbonate, which was in there.