Measures of Concentration: Molarity — Unit test

Question 1

A student prepares 150.0 mL of 1.40 M HCl using 35.0 mL of a stock solution. What is the concentration of the stock solution?Use .

Revolt · Accepted Answer

6.00 M

Question 2

Which solution is the most concentrated?

Revolt · Accepted Answer

2.0 mL of 10.5 M H2O2, where H2O2 has a molar mass of 34 g/mol

Question 3

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

Revolt · Accepted Answer

0.50 mol

Question 4

Given that the molar mass of NaOH is 40.00 g/mol, what mass of NaOH is needed to make 2.500 L of a 2.000 M NaOH solution?Use .

Revolt · Accepted Answer

200.0 g

Question 5

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?

Revolt · Accepted Answer

0.50 M

Question 6

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 .

Revolt · Accepted Answer

0.400 M

Question 7

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?Use .

Revolt · Accepted Answer

6.94 mL

Question 8

Which is a way to express concentration of a solution?

Revolt · Accepted Answer

parts per billion

Question 9

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 .

Revolt · Accepted Answer

0.300 M

Measures of Concentration: Molarity — Unit test Answers

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