Dilutions Worksheet
1)
If 45 mL of water are added to 250 mL of a 0.75 M K2SO4 solution, what will the
molarity of the diluted solution be?
2)
If water is added to 175 mL of a 0.45 M KOH solution until the volume is 250 mL, what
will the molarity of the diluted solution be?
3)
How much 0.075 M NaCl solution can be made by diluting 450 mL of 9.0 M NaCl?
4)
If 550 mL of a 3.50 M KCl solution are set aside and allowed to evaporate until the
volume of the solution is 275 mL, what will the molarity of the solution be?
5)
How much water would need to be added to 750 mL of a 2.8 M HCl solution to make a
1.0 M solution?
Dilutions Worksheet – Solutions
1)
If 45 mL of water are added to 250 mL of a 0.75 M K2SO4 solution, what will the
molarity of the diluted solution be?
(0.75 M)(250 mL) = M2 (295 mL)
M2 = (0.75 M)(250 mL) = 0.64 M
(295 mL)
2)
If water is added to 175 mL of a 0.45 M KOH solution until the volume is 250 mL, what
will the molarity of the diluted solution be?
(0.45 M)(175 mL) = M2 (250 mL)
M2 = (0.45 M)(175 mL) = 0.32 M
(250 mL)
3)
How much 0.075 M NaCl solution can be made by diluting 450 mL of 9.0 M NaCl?
(9.0 M)(450 mL) = (0.075 M)V2
V2 = (9.0 M)(450 mL) = 54,000 mL = 54 L
(0.075 M)
4)
If 550 mL of a 3.50 M KCl solution are set aside and allowed to evaporate until the
volume of the solution is 275 mL, what will the molarity of the solution be?
(3.50 M)(550 mL) = M2 (275 mL)
M2 = (3.50 M)(550 mL) = 7.0 M
(275 mL)
5)
How much water would need to be added to 750 mL of a 2.8 M HCl solution to make a
1.0 M solution?
(2.8 M)(750 mL) = (1.0 M)V2
V2 = (2.8 M)(750 mL) = 2100 mL
(1.0 M)
2100 mL – 750 mL = 1350 mL = 1.4 L
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