Assignment

1. Write balanced complete ionic and net ionic equations for each acid-base reaction.

a. HBr(aq) + NaOH(aq) →
b. HF(aq) + NaOH(aq) →
c. HC₂H₃O₂(aq) + RbOH(aq) →

2. Write balanced complete ionic and net ionic equations for each add-base reaction.

a. HI(aq) + RbOH(aq) →
b. HCHO₂(aq) + NaOH(aq) →
c. HC₂H₃O₂(aq) + LiOH(aq) →

3. Complete and balance each combustion reaction equation.

a. S(s) + O₂(g) →
b. C₃H₆(g) + O₂(g) →
c. Ca(s) + O₂(g) →
d. C₅H₁₂S(l) + O₂(g) →

4. Complete and balance each combustion reaction equation.

a. C₄H₆(g) + O₂(g) →
b. C(s) + O₂(g) →
c. CS₂(s) + O₂(g) →
d. C₃H₈O(l) + O₂(g) →

5. The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C₈H₁₈) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

6. Many home barbeques are fueled with propane gas (C₃H₈). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid.

7. A solution contains one or more of the following ions: Ag⁺, Ca²⁺ and Cu²⁺ . When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Which ions were present in the original
solution? Write net ion equations for the formation of each of the precipitates observed.

8. A solution contains one or more of the following ions: Hg₂²⁺, Ba²⁺, and Fe²⁺. When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Which ions were present in the original solution? Write net ionic equations for the formation of each of the precipitates observed.