1.Calculate the molar mass of barium hydrogen sulfate.
2.Calculate the mass of 3.5 moles of sulfuric acid.
3.How many moles of hydrochloric acid are in 3kg of 5% acid.
4. A 12.33% nitric acid solution has a density of 1.070 g / cm 3 . Calculate the mass of 3 l of this solution, then the number of moles of nitric acid found there.
5.Calculate the mass of one liter of a sulfuric acid solution to 98.52% (density of this solution = 1.8405)
, then the number of moles which are in one liter (that is 'call molarity).
6. A solution containing 1.465 g / cm3 of sulfuric acid has a density of 1.765 g / cm 3 . Calculate the mass of one liter of this solution, then the percentage of acid contained in one liter of this solution.
7. A 4.84 molar solution (containing 4.84 mol per liter) of hydrochloric acid has a density of 1.065. Calculate the volume of 100 g of solution, then the mass of acid in it.
8. A 10% solution of perchloric acid has a density of 1.0597. Calculate the molarity of this solution (molarity = number of moles per liter).
9.Calculate the percentage (mass per 100 g) of iodine in a 1.0751 g / cm 3 solution of hydroiodic acid with a molarity equal to 0.841 mol / l.
What mass of barium sulfate can be precipitated from 10 g of a 5% solution of barium hydroxide and an excess of sulfuric acid.
11. Calculate the mass of calcium hydroxide obtainable from 40 g of quicklime (calcium oxide), then calculate the volume that should have a 0.01 molar solution (mole per liter) of this hydroxide.
12. Sodium is burned in the air and the oxide obtained is introduced into the water. What mass of sodium was burned, if finally available 2 L of 0.2 molar solution of sodium hydroxide (sodium hydroxide).
13. What volume of 0.1 molar solution of silver nitrate was used to form 2 g of precipitate by adding an excess of cooking salt solution.
14. From 100 ml of a potassium carbonate solution, 0.134 mol of carbon dioxide was obtained. Calculate the molarity of the potassium carbonate solution and the mass of potassium carbonate therein.