Lesson 7: Measures of Concentration: Molarity Quiz

A chemistry teacher adds 50.0 mL of 1.50 M H2SO4 solution to 200 mL of water. What is the concentration of the final solution?

0.300 M

A stock solution is made by dissolving 66.05 g of (NH4)2SO4 in enough water to make 250 mL of solution. A 10.0 mL sample of this solution is then diluted to 50.0 mL. Given that the molar mass of (NH4)2SO4 is 132.1 g/mol, what is the concentration of the new solution?

0.400 M

A chemist uses 0.25 L of 2.00 M H2SO4 to completely neutralize a 2.00 L of solution of NaOH. The balanced chemical equation of the reaction is given below. 2NaOH+H2SO4-->Na2SO4+2H2O What is the concentration of NaOH that is used?

0.50 M

How many moles of Ba(NO3)2 are there in 0.25 L of a 2.00 M Ba(NO3)2 solution?

0.50 mol

In a group assignment, students are required to fill 10 beakers with 0.720 M CaCl2. If the molar mass of CaCl2 is 110.98 g/mol and each beaker must have 250. mL of solution, what mass of CaCl2 would be used?

200 g

In a school's laboratory, students require 50.0 mL of 2.50 M H2SO4 for an experiment, but the only available stock solution of the acid has a concentration of 18.0 M. What volume of the stock solution would they use to make the required solution?

6.94 mL

Which is a way to express concentration of a solution?

Parts per billion

Which would be the best way to represent the concentration of a 1.75 M K2CrO4 solution?

[K2CrO4]