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Honors Chemistry Name _______________________ Concentrations of Solutions Date ________________________ Complete the following problems on a separate sheet of paper. Use significant figures.
Note: The density of water is 1 g/mL.
1. What is the molarity of a solution that contains 10.0 grams of Silver Nitrate that has been dissolved in 750 mL of water?
10.0 π π΄πππ!
1 π₯
1 ππππ π΄πππ!169.872 π π΄πππ!
= 0.0588678 πππππ π΄πππ!
π = π
π (ππ πΏ) =
0.0588678 πππππ π΄πππ!0.75 πΏ
= 0.078 π π΄πππ!
2. You want to create a 0.25 M Potassium Chloride solution. You mass 5.00 grams of Potassium
Chloride. How much water is needed?
5.00 π πΎπΆπ1
π₯ 1 ππππ πΎπΆπ74.551 π πΎπΆπ
= 0.067068 πππππ πΎπΆπ
π =
ππβ π πππ£π πππ π£πππ’ππ
π = ππ= 0.067068 πππππ πΎπΆπ
0.25 π πΎπΆπ= 0.27 πΏ = 270 ππΏ
3. What is the molality of a solution that contains 48 grams of sodium chloride and 250 mL of
water?
48 π πππΆπ1
π₯ 1 ππππ πππΆπ58.443 π πππΆπ
= 0.8213 πππππ πππΆπ
250 ππΏ π»!π
1 π₯
1 π π»!π1 ππΏ π»!π
π₯ 1 ππ π»!π1000 π π»!π
= 0.25 ππ π»!π
πππππππ‘π¦ = πππππ π πππ’π‘πππ π πππ£πππ‘
= 0.8213 πππππ πππΆπ
0.25 ππ π»!π= 3.3 π πππΆπ
4. What is the percentage by mass of the solution from problem 1?
750 ππΏ π»!π
1 π₯
1 π π»!π1 ππΏ π»!π
= 750 π π»!π
πππππππ‘ ππ¦ πππ π = πππ π ππ π πππ’π‘ππππ π ππ π πππ’π‘πππ
π₯ 100 = 10.0 π π΄πππ!10.0 π + 750 π
π 100 = 1.32 π΄πππ!
5. How many mL of hydrogen peroxide are needed to make a 8.5% solution by volume of hydrogen
peroxide if you want to make 450 mL of solution?
πππππππ‘ ππππ’ππ = π£πππ’ππ ππ π πππ’π‘ππ£πππ’ππ π πππ’π‘πππ
π₯ 100
2
ππππ’ππ ππππ’π‘π = πππππππ‘ ππππ’ππ π₯ ππππ’ππ ππππ’π‘πππ
100= (8.5%)(450 ππΏ)
100= 38 ππΏ π»!π!
6. What is the mole fraction of the solute in the solution from problem 1?
750 ππΏ π»!π
1 π₯
1 π π»!π1 ππΏ π»!π
π₯ 1 ππππ π»!π18.015 π π»!π
= 41.63197 ππππ π»!π
π!"#$%& = πππππ π πππ’π‘ππππππ π πππ’π‘πππ
= 0.0588678 πππππ π΄πππ!
0.0588678 πππππ π΄πππ! + 41.63197 ππππ π»!π= 0.0014
7. What is the mole fraction of the solvent in the solution from problem 1?
π!"#$%&' = πππππ π πππ£πππ‘πππππ π πππ’π‘πππ
= 41.63197 ππππ π»!π
0.0588678 πππππ π΄πππ! + 41.63197 ππππ π»!π= 1.0
8. What is the molality of the ions in the solution from problem 3?
3.3 π πππΆπ = 0.82131 πππππ πππΆπ
0.25 ππ π»!π
1 ππππ πππΆπ = 2 πππππ ππππ
0.82131 πππππ πππΆπ
0.25 ππ π»!π π₯ 2 πππππ πππΆπ ππππ
1 ππππ πππΆπ= 6.6 π πππΆπ ππππ
9. What is the molality of a solution that contains 13.4 grams of calcium chloride dissolved in 655
mL of water?
13.4 π πΆππΆπ!1
π₯ 1 ππππ πΆππΆπ!
110.986 π πΆππΆπ!= 0.1207359 πππππ πΆππΆπ!
655 ππΏ π»!π
1 π₯
1 π π»!π1 ππΏ π»!π
π₯ 1 ππ π»!π1000 π π»!π
= 0.655 ππ π»!π
πππππππ‘π¦ = πππππ π πππ’π‘πππ π πππ£πππ‘
= 0.1207359 πππππ πΆππΆπ!
0.655 ππ π»!π= 0.184 π πΆππΆπ!
10. What is the molality of the ions in the solution from problem 9?
0.1207359 πππππ πΆππΆπ!
0.655 ππ π»!π= 0.184 π πΆππΆπ!
1 ππππ πΆππΆπ! = 3 πππππ πΆππΆπ! ππππ
0.1207359 πππππ πΆππΆπ!
0.655 ππ π»!π π₯ 3 πππππ πΆππΆπ! ππππ
1 ππππ πΆππΆπ!= 0.553 π πΆππΆπ! ππππ