AP Chemistry  Solution Molarity Worksheet 
1. 
Suppose you prepare a 0.200 M salt solution in a 250mL
volumetric flask and then accidentally spill some of it. What happens to
the concentration of the solution in the bottle?

2. 
Calculate the number of grams of each solute that has
to be taken to make each of the following solution. 

(a) 250 mL of 0.100 M NaCl 

(b) 100 mL of 0.440 M C_{6}H_{12}O_{6}
(glucose) 

(c) 500 mL of 0.500 M H_{2}O_{2
} 
3. 
How much solute, in grams, is needed to make each of
the following solutions? 

(a) 250 mL of 0.00100 M Na_{2}SO_{4} 

(b) 100 mL of 0.250 M Na_{2}CO_{3} 

(c) 500 mL of 0.400 M NaOH

4. 
What is the molarity of pure water?

5. 
Concentrated ammonia contains 26 grams NH_{3}
per 100 mL of solution. What is its molarity?

6. 
What is the molarity of a solution of sodium chloride
that contains 26.00 g NaCl/100.0 mL solution?

7. 
What is the molarity of a solution prepared by disoolving
17.1 grams of ordinary sugar (C_{12}H_{22}O_{11})
in enough water to make 0.500 L of solution?

8. 
What is the molarity of a solution made by dissolving
10.0 grams of NaOH in 0.200 L of water?

9. 
Calculate the molarity of a solution containing 5.0
mg of BaCl_{2} per mL of solution.

10. 
Calculate the grams of silver nitrate needed to prepare
0.500 L of a 0.100 M solution.

11. 
Calculate the grams of BaCl_{2} needed to prepare
200 mL of a 0.500 M solution.

12. 
The following questions refer to a 0.20 M solution
of BaCl_{2}. The molecular mass of BaCl_{2} is 208.23 g/mole.


a) Calculate the moles of BaCl_{2} in 2.00
mL of solution. 

b) Calculate the mg and grams of BaCl_{2} in
2.00 mL of the solution. 

c) Calculate the volume in mL that contains 5.0 moles
of BaCl_{2}. 

d) Calculate the volume in mL that contains 41.6 mg
of BaCl_{2}.

13. 
Calculate 

a) the volume of 2.0 M CaCl_{2} that must be
used to prepare 1200 mL of 0.80 M CaCl_{2} 

b) the volume of water that must be added.

14. 
Calculate the molarity of these solutions: 

a) 1.00 L containing 119 grams of KCl 

b) 2.00 L containing 223.5 grams of CuBr_{2} 

c) 0.250 L containing 13.35 grams of aluminum chloride 

d) 0.150 L containing 13.0 grams cobalt(II) chloride 

e) 0.250 L containing 4.33 grams of chromium(III) iodide

15. 
How many moles of NaOH are contained in 

a) 1.0 litre of a 1.0 M solution? 

b) 0.50 L of a 1.0 M solution? 

c) 0.50 L of a 0.50 M solution? 

d) 0.125 L of a 0.50 M solution? 

e) 5.0 x 10^{2} L of a 5.0 x 10^{3}
M solution

16. 
Calculate the mass of solute needed to make these solutions: 

a) 1.0 L of 1.0 M sodium hydroxide 

b) 0.500 L of 2.00 M calcium nitrate 

c) 2.0 L of 0.50 M potassium bromide 

d) 0.200 L of 0.75 M zinc chloride 

e) 0.125 L of 2.40 M ammonium chloride

17. 
What mass of solute is required to prepare the volume
of each of these solutions? 

a) 500 mL of 3 M CaCl_{2}? 

b) 750 mL of 2.0 M H_{2}SO_{4}? 

c) 5.0 L of 0.50 M H_{2}C_{2}O_{4}? 

d) 0.125 L of 8.00 M HC_{2}H_{3}O_{2}? 

e) 5.0 x 10^{4} mL of 0.10 M KBr? 

f) 1.0 x 10^{3} L of 1.0 x 10^{3}
M NH_{4}Cl? 

g) 150 mL of 0.50 M ZnCl_{2}?

18. 
Tell how to prepare a solution of HNO_{3} which
contains 0.1 mmol per mL from a 6 M stock solution of HNO_{3
} 
19. 
Fifty mL of 0.50 M HCl is mixed with 30 mL of 0.28
M HCl. Calculate the molarity of the resulting mixture.

20. 
Two litres of 6.0 M HNO_{3} is added to 1.0
L of 2.0 M HNO_{3}. What is the concentration of HNO_{3} in
the mixture?

21. 
Calculate the volume of 12 M HCl that must be added
to 2.5 L of 1.0 M HCl in order to obtain 15 L of 1.0 M HCl.

22. 
50.0 mL of an aqueous NaCl solution yielded 1.25 grams
NaCl on evaporation. What was the molarity of the original solution.

23. 
Calculate the molarity of a solution prepared by dissolving
54.5 grams of Na_{2}CO_{3}^{.}10H_{2}O in
enough water to give the resulting solution a volume of 2.4 L.

24. 
What volume of 2.00 mol/L HNO_{3} is needed
to yield 10.00 grams of HNO_{3}?

25. 
Give directions for preparing 500 mL of 0.050 mol/L
KMnO_{4}.

26. 
Give directions for preparing 250 mL of 0.500 mol/L
CuSO_{4} using CuSO_{4}^{.}5H_{2}O as solute. 