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Worksheet: Molarity Name______________

CHEMISTRY: A Study of Matter

© 2004, GPB

10.18a KEY

Molarity:

• a _______________ description of solution concentration. • Abbreviated _______________

Molarity = ________________

Problems: Show all work and circle your final answer.

1. To make a 4.00 M solution, how many moles of solute will be needed if 12.0

liters of solution are required?

4.00 M = moles of solute

12.0 L moles of solute = 48.0 mol

2. How many moles of sucrose are dissolved in 250 mL of solution if the solution

concentration is 0.150 M? ? L = 250 mL × 1 L

1000 mL = 0.25 L

0.150 M = moles of solute

0.25 L moles of solute = 0.038 mol

3. What is the molarity of a solution of HNO3 that contains 12.6 grams HNO3 in

1.0 L of solution?

? mol HNO3 = 12.6 g HNO3 × 1 m o l H N O3

63.0 g HNO

3 = 0.200 mol HNO3

M = 0.200 mol HNO3

1.0 L = 0.200 M

4. How many grams of potassium nitrate are required to prepare 0.250 L of a

0.700 M solution?

0.700 M = moles of solute

0.250 L moles of solute = 0.175 mol

? g KNO3 = 0.175 mol KNO3

× 101.1 g KNO3

1 mol KNO

3 = 17.7 g KNO3

quantitative M moles of solute liters of solution

CHEMISTRY: A Study of Matter

© 2004, GPB

10.18b 5. 125 cm3 of solution contains 3.5 moles of solute. What is the molarity of the

solution? ? g KNO3 = 0.175 mol KNO3 × 101.1 g KNO3

1 mol KNO

3 = 17.7 g KNO3

M = 3.5 mol

0.125 L = 28 M

6. Which solution is more concentrated? Solution "A" contains 50.0 g of CaCO3 in

500.0 mL of solution. Solution "B" contains 6.0 moles of H2SO4 in 4.0 L of

solution.

SHOW WORK!

? mol CaCO3 = 50.0 g CaCO3 × 1 mol CaCO3

100.0 g CaCO

3 = 0.500 mol CaCO3

? L = 500.0 mL

× 1 L

1000 mL = 0.500 L M = 0.500 mol

0.500 L = 1.00 M

M = 6.0 mol

4.0 L = 1.5 M

7. How many liters of solution can be produced from 2.5 moles of solute if a 2.0 M

solution is needed?

2.0 M = 2.5 moles

liters of solution liters of solution = 1.25 L = 1.3 L

8. What would be the concentration of a solution formed when 1.00 g of NaCl are

dissolved in water to make 100.0 mL of solution? ? mol = 1.00 g NaCl × 1 mol NaCl

58.5 g NaCl = 0.0171 mol NaCl

? L = 100.0 mL × 1 L

1000 mL

= 0.1000 L M = 0.0171 mol

0.1000 L = 0.171 M

"A": "B": "B" is more concentrated: 1.5 Mquotesdbs_dbs3.pdfusesText_6