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AP Chemistry
Solution Concentration Assignment

1.   A solution is prepared by dissolving 50.0 g cesium choride (CsCl) in 50.0 g water. The volume of
the solution is 63.3 cm3. Calculate the mass percent, molarity, molality and mole fraction of the
cesium chloride.

2.   Household vinegar is an aqueous 5.0% acetic acid solution (by mass). If the density of household
vinegar is 1.01 g/mL, calculate the mole fraction, molarity, and molality of the solution.

3.   A solution is prepared by mixing 50.0 mL toluene (C6H5CH3, d = 0.867 g/cm3) with 125 mL
benzene (C6H6, d = 0.874 g/cm3). Assuming that the volumes add upon mixing, calculate the mass
percent, mole fraction, molality, molarity of the toluene.

4.   A bottle of wine contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is
0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molarity.

5.   A 1.37 M solution of citric acid (H3C6H5O7) in water has a density of 1.10 g/cm3. Calculate the
mass percent, molality and mole fraction. Citric acid has 3 acidic protons.

6.   Calculate the molarity and mole fraction of acetone in a 1.00m solution of acetone (CH3COCH3,
d = 0.788 g/cm3) in ethanol. Assume the volumes of acetone and ethanol add.

7.   An aqueous antifreeze solution is 40.0% ethylene glycol (C2H6O2) by mass. The density of the
solution is 1.05 g/cm3. Calculate the molality, molarity, and mole fraction of the ethylene glycol
solution.

8.   The units parts per million (ppm) and parts per billion (ppb) are commonly used by environmental
chemists to describe the concentration of very dilute aqueous solutions. Calculate the molarity of
each of the following aqueous solutions:
a) 5.0 ppb Hg in H2O
b) 0.10 ppm DDT (C14H9Cl5) in H2

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