CHEM 3: Solutions and Concentrations
1.
An experiment calls for 25.00 mL of an aqueous solution containing a concentration of 0.1924 M chloride ion,
[Cl-] = 0.1924 M. What mass of magnesium chloride (in grams) would be needed to produce this
concentration of chloride ion?
2.
Consider an aqueous solution prepared by dissolving 5.992 g of silver (I) sulfate into a volumetric flask
containing a final solution volume of100.0 mL.
 What is the molarity (M = mol/L) of sulfate ion in this solution?

What is the molarity (M = mol/L) of silver ion in this solution?
3.
A chemical reaction calls for 30.00 mL of an aqueous sodium hydroxide solution with a concentration of 20.00
% by mass. If this aqueous solution has a density of 1.219 g/mL, what is the concentration of the sodium
hydroxide expressed in units of molarity (mol/L)?
4.
An aqueous solution is prepared by adding 0.493 g of lead (II) nitrate to 1.00 L of water. Assuming the density
of water is 0.996 g/mL, calculate the final concentration of lead ions in parts per million.
5.
A solution of hexavalent chromium (Cr6+ ions) was found to have a chromium ion concentration of 1.592 x 105
M (mol/L). If the solution has a density of 0.9969 g/mL, what is the equivalent concentration of chromium
ions in parts per million (ppm)?
6.
Consider the reaction of aqueous lead (II) nitrate with aqueous sodium chloride.
What volume of 0.9227 M aqueous sodium chloride (in mL) would be needed to fully react with 10.0 mL of
0.4529 M aqueous lead (II) nitrate?