SCH3U ~ Shirzadi
Date: __________________
Molarity Calculations
Find the molarity of the following solutions: (1-5)
1. 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution.
2. 0.5 grams of sodium chloride is dissolved to make 0.05 liters of solution.
3. 0.5 grams of sodium chloride is dissolved to make 0.05 mL of solution.
4. 734 grams of lithium sulfate are dissolved to make 2500 mL of solution.
5. 6.7 x 10-2 grams of Pb(C2H3O2)4 are dissolved to make 3.5 mL of solution.
6. Consider two solutions: In the first solution, 1.0 moles of sodium chloride is dissolved to make 1.0
liters of solution. In the second one, 1.0 moles of sodium chloride is added to 1.0 liters of water. Is
the molarity of each solution the same? Explain your answer.
7. How many grams of beryllium chloride are needed to make 125 mL of a 0.050 M solution?
8. The density of ethanol is 0.789 g/mL. How many grams of ethanol should be mixed with 225 mL of
water to make a 4.5% (v/v) mixture?
9. Explain how to make at least one liter of a 1.25 M ammonium hydroxide solution.
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10. What is the molarity of a solution in which 0.45 grams of sodium nitrate are dissolved in 265 mL of
solution?
11. What will the volume of a 0.50 M solution be if it contains 25 grams of calcium hydroxide?
12. How many grams of ammonia are present in 5.0 L of a 0.050 M solution?
13. If you add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the
diluted solution be?
For these questions you will have to use the formula: C1∙V1 = C2∙V2
14. If you add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will
the molarity of the diluted solution be?
15. How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?
16. You have 345 mL of a 1.5 M NaCl solution. If you boil the water until the volume of the solution is
250 mL, what will the molarity of the solution be?
17. How much water would you need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M
solution?
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Solutions to the Molarity Practice Worksheet
For the first five problems, you need to use the equation that says that the molarity of a solution is equal to
the number of moles of solute divided by the number of liters of solution.
1)
In this problem, simply solve using the molarity equation to find that the concentration of the
solution is 10 M.
2)
To use the molarity equation, you need to convert grams of sodium chloride to moles of sodium
chloride before you can use the molarity equation. Because you have 0.0085 moles of NaCl in this
solution, the total concentration is 0.17 M.
3)
To use the molarity equation, you need to convert grams of NaCl to moles and mL of solution to
liters. When you do this, the total concentration of the solution is 170.9 M. As it turns out, this isn’t
a realistic value for molarity, so you’d never see a solution with this concentration out in the real
world. Why did I give it to you then? I did it because I wanted you to see that just by changing a
few units, you can get very different final answers.
4)
This is done in the same method that you’d solve #3. Because you have 6.68 moles of Li2SO4 and
2.500 liters of water, the overall molarity of your solution is 2.67 M.
5)
This problem is also solved in the same way as #3 and #4. Because you have 1.51 x 10-4 moles of
Pb(C2H3O2)4, and 0.0035 L of water, the total concentration is 4.32 x 10-2 M, or 0.0432 M.
6)
The equation for molarity states that the molarity of a solution is equal to the number of moles of
solute divided by the number of liters of solution. In the first equation, the molarity will clearly be
equal to 1.0 M, because there are 1.0 moles of NaCl and a solution volume of 1.0 L. In the second
solution, the molarity will be different, because the solution volume will be greater than 1.0 liters.
Why? If you already have 1.0 L of water and add 1.0 moles of salt to it, it will overflow, right? This
is because the volume will be (roughly) equal to the volume of the water plus the volume of the salt,
which will be greater than 1.0 L. It is for this reason that when you make a solution, you always
dissolve the solute in only a little bit of water and then add water to make your final volume.
7)
How many grams of beryllium chloride are needed to make 125 mL of a 0.050 M solution?
0.50 grams
9)
The density of ethanol is 0.789 g/mL. How many grams of ethanol should be mixed with 225 mL of
water to make a 4.5% (v/v) mixture?
7.99 grams
10)
Explain how to make at least one liter of a 1.25 molal ammonium hydroxide solution.
Dissolve 43.8 grams (1.25 moles) of ammonium hydroxide in 1 L H2O.
11)
What is the molarity of a solution in which 0.45 grams of sodium nitrate are dissolved in 265 mL of
solution?
0.020 M
12)
What will the volume of a 0.50 M solution be if it contains 25 grams of calcium hydroxide?
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680 mL
13)
How many grams of ammonia are present in 5.0 L of a 0.050 M solution?
4.5 grams
14)
If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted
solution be?
M1V1 = M2V2
(0.15 M)(125 mL) = x (150 mL)
x = 0.125 M
15)
If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the
molarity of the diluted solution be?
M1V1 = M2V2
(0.15 M)(100 mL) = x (150 mL)
x = 0.100 M
16)
How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?
M1V1 = M2V2
(10 M)(250 mL) = (0.05 M) x
x = 50,000 mL
17)
I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250
mL, what will the molarity of the solution be?
M1V1 = M2V2
(1.5 M)(345 mL) = x (250 mL)
x = 2.07 M
18)
How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?
M1V1 = M2V2
(2.4 M)(500 mL) = (1.0 M) x
x = 1200 mL
1200 mL will be the final volume of the solution. However, since there’s already 500 mL of
solution present, you only need to add 700 mL of water to get 1200 mL as your final volume.
The answer: 700 mL.
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