Table 1: Summary of Solubility Rules
Rule
Soluble
Insoluble
Nitrate (NO3-)
Chlorate (ClO3-)
1
Perchlorate (ClO4-)
N/A
Acetate (CH3COO-)
N/A
2
Chloride (Cl-)
3
Bromide (Br-)
Iodide (I-)
Magnesium (Mg2+)
Calcium (Ca2+)
Strontium (Sr2+)
4
Barium (Ba2+)
Lead (II) (Pb2+)
5
Sulfate (SO42-)
Group 1 Alkali Metal Cations
6
Group 2 Alkaline Earth Metal Cations
Ammonium (NH4+)
Carbonate (CO32-)
Phosphate (PO43-)
7
Chromate (CrO2-)
Group 1 Alkali Metal Cations
8
Ammonium (NH4+)
*Ba(OH)2, Ca(OH)2, Sr(OH)2 somewhat soluble
Solution Stoichiometry
1. Lead (II) iodide can be produced form the reaction of lead (II) nitrate and potassium iodide.
a. Write the balanced chemical equation for the reaction.
b. What mass of lead (II) iodide produced when 50.0 mL of 0.500 M lead (II) nitrate is mixed with 75.0
mL of 0.750 M potassium iodide?
2. The active ingredient in Milk of Magnesia, a commonly used laxative, is magnesium hydroxide. A 10.0 mL
sample of Milk of Magnesia was analyzed and required 18.26 mL of 1.50 hydrochloric acid for complete
neutralization.
a. Write out balanced chemical equation for the reaction between hydrochloric acid and magnesium
hydroxide.
b. Calculate the mass (in mg) of magnesium hydroxide present in the sample of Milk of Magnesia.
c. Calculate the mass percent concentration of magnesium hydroxide in Milk of Magnesia given that
the density of Milk of Magnesia is 1.1 g/mL.
3. I have 345 mL of 1.5 M NaCl solution. If I boil the water until the volume of solution is 250 mL, what will
the molarity of the solution be?
4. How much water would I need to add to 500 mL of 2.4 M KCl solution to make a 1.0 M solution?
5. Titration reveals that 11.6 mL of 3.0 M sulfuric acid are required to neutralize the sodium hydroxide in
25.00 mL of NaOH solution. What is the molarity of the NaOH solution?
1. Lead (II) iodide can be produced form the reaction of lead (II) nitrate and potassium iodide.
a. Write the balanced chemical equation for the reaction.
b. What mass of lead (II) iodide produced when 50.0 mL of 0.500 M lead (II) nitrate is mixed with 75.0
mL of 0.750 M potassium iodide?
2. The active ingredient in Milk of Magnesia, a commonly used laxative, is magnesium hydroxide. A 10.0 mL
sample of Milk of Magnesia was analyzed and required 18.26 mL of 1.50 hydrochloric acid for complete
neutralization.
a. Write out balanced chemical equation for the reaction between hydrochloric acid and magnesium
hydroxide.
b. Calculate the mass (in mg) of magnesium hydroxide present in the sample of Milk of Magnesia.
c. Calculate the mass percent concentration of magnesium hydroxide in Milk of Magnesia given that
the density of Milk of Magnesia is 1.1 g/mL.
3. I have 345 mL of 1.5 M NaCl solution. If I boil the water until the volume of solution is 250 mL, what will
the molarity of the solution be?
4. How much water would I need to add to 500 mL of 2.4 M KCl solution to make a 1.0 M solution?
5. Titration reveals that 11.6 mL of 3.0 M sulfuric acid are required to neutralize the sodium hydroxide in
25.00 mL of NaOH solution. What is the molarity of the NaOH solution?
Table 1: Summary of Solubility Rules
Rule
Soluble
Insoluble
Nitrate (NO3-)
Chlorate (ClO3-)
1
Perchlorate (ClO4-)
N/A
Acetate (CH3COO-)
Group 1 Cations
2
3
Ammonium Ions (NH4+)
N/A
Chloride (Cl-)
Silver (Ag+)
Bromide (Br-)
Lead (II) (Pb2+)
Iodide (I-)
Mercury (Hg22+)
Magnesium (Mg2+)
Calcium (Ca2+)
4
Fluoride (F-)
Strontium (Sr2+)
Barium (Ba2+)
Lead (II) (Pb2+)
Silver (Ag+)
Calcium (Ca2+)
5
Sulfate (SO42-)
Strontium (Sr2+)
Barium (Ba2+)
Lead (II) (Pb2+)
Group 1 Alkali Metal Cations
6
Group 2 Alkaline Earth Metal Cations
Sulfide (S2-)
Ammonium (NH4+)
Carbonate (CO32-)
Group 1 Alkali Metal Cations
7
Ammonium (NH4+)
Group 1 Alkali Metal Cations
8
Phosphate (PO43-)
Chromate (CrO2-)
Hydroxide (OH-)
+
Ammonium (NH4 )
*Ba(OH)2, Ca(OH)2, Sr(OH)2 somewhat soluble
Oxide (O2-)
Solution Stoichiometry
1. Lead (II) iodide can be produced form the reaction of lead (II) nitrate and potassium iodide.
a. Write the balanced chemical equation for the reaction.
b. What mass of lead (II) iodide produced when 50.0 mL of 0.500 M lead (II) nitrate is mixed with 75.0
mL of 0.750 M potassium iodide?
2. The active ingredient in Milk of Magnesia, a commonly used laxative, is magnesium hydroxide. A 10.0 mL
sample of Milk of Magnesia was analyzed and required 18.26 mL of 1.50 hydrochloric acid for complete
neutralization.
a. Write out balanced chemical equation for the reaction between hydrochloric acid and magnesium
hydroxide.
b. Calculate the mass (in mg) of magnesium hydroxide present in the sample of Milk of Magnesia.
c. Calculate the mass percent concentration of magnesium hydroxide in Milk of Magnesia given that
the density of Milk of Magnesia is 1.1 g/mL.
3. I have 345 mL of 1.5 M NaCl solution. If I boil the water until the volume of solution is 250 mL, what will
the molarity of the solution be?
4. How much water would I need to add to 500 mL of 2.4 M KCl solution to make a 1.0 M solution?
5. Titration reveals that 11.6 mL of 3.0 M sulfuric acid are required to neutralize the sodium
hydroxide in 25.00 mL of NaOH solution. What is the molarity of the NaOH solution?