Problem Set 10
(Due November 7)
Name_______________________________
Suggested Book Problems: 13.21, 13.23, 13.25, 13.29, 13.31, 15.17, 15.19, 13.71, 13.73, 13.75,
13.79, 13.81, 13.103, 13.105, 13.107, 13.113, 13.115, 13.119, 13.121, 13.123, 13.125
1. Which of the following compounds are soluble in aqueous solution?
NaNO3
Lead iodide
C8H18
CH3OH
Magnesium sulfide
AgNO3
AgCl
(NH4)3PO4
Manganese (II) sulfide
Ca(OH)2
KCl
Silver acetate
2. Write balanced ionic and net ionic equations for each of the following single or double replacement
reactions that occur in aqueous solution. Make sure to consider solubility rules and include phases in
your answer. RECALL THAT CATIONS AND ANIONS PAIR UP, NOT CATIONS AND CATIONS OR
ANIONS AND ANIONS.
a. CaCl2 + CuSO4 
b. Ca(NO3)2 + K2CO3 
c. Mg + HBr 
d. (NH4)2SO4 + NaBr 
3. Calculate how many moles, grams, and atoms of sodium is present in each of the following solutions:
a. 1.00 L of 1.00 M NaCl
b. 3.86 L of 1.8M Na2CO3
c. 1.00 L of 1.00 mM NaF
d. 45.89 mL of 56.89 mM sodium oxide.
4. For each of the following solutions, determine the volume that contains exactly 6.022 x 1023 atoms of
chlorine.
a. 1.00 M NaCl
b. 0.985 M MgCl2
c. 36.84 nM KClO4
5. What is the molarity of a solution prepared by adding 1.85 L of water to 1.85 grams of potassium
phosphate?
6. 34.8 mL of 1.86 M HCl is diluted to a concentration of 1.86 mM.
a. What is the volume of the solution after the dilution?
b. How much water do you need to add to make this solution?
7. 3L of 0.68M NaCl is mixed with 2.87 L of 0.44 M AgNO3
a. Write a balanced net ionic equation for this reaction.
b. Determine the concentration of aqueous Na+ after the two solutions have mixed and reacted.
c. Assuming 100% yield, determine the mass of any solid product that forms.
8. Consider the following chemical reaction:
2 HNO3 (aq) + Sn (s)  Sn(NO3)2 (aq) + H2 (g)
a. What volume of 1.8 M nitric acid is required to react with 116 grams of tin?
b. What volume of H2 at STP would be produced if 1L of 1M nitric acid reacts with 100 grams of
tin?
3a. 1 mol, 22.99 g, 6.022 x 1023 atoms b. 13.896 mol, 319.47 g, 8.37 x 1024 atoms c. 0.001 mol, .02299 g, 6.022 x 1020 atoms
d. 0.005221 mol, 0.12 g, 3.144 x 1021 atoms
4. a 1L b. 0.5076 L c. 2.71 x 107 L 5. 4.71 mM
6a. 34.8 L b. 34765.2 mL
7. B. 0.348 M c. 181.01 g
8a. 1.086 L b. 18.89 L