Honors Chem Semester 2 Molarity

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?Use .

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?Use and .

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 + 2H2OWhat is the concentration of NaOH that is used?

0.50 M

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?Use .

200 g

A student takes a measured volume of 3.00 M HCl to prepare a 50.0 mL sample of 1.80 M HCl. What volume of 3.00 M HCl did the student use to make the sample?Use .

30.0 mL

Given that the molar mass of NaNO3 is 85.00 g/mol, what mass of NaNO3 is needed to make 4.50 L of a 1.50 M NaNO3solution?Use .

574 g

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

[K2CrO4]

Which is a way to express concentration of a solution?

parts per billion

Which best defines concentration?

ratio that describes the amount of solute divided by the amount of solvent or solution

Josh prepares a solution by mixing sodium nitrate and water. To calculate the molarity of the solution, Josh should calculate the moles of which substance, and why?

sodium nitrate, because it is the solute