Chapters 8 & 9 Study Questions
1. Sodium carbonate and iron(III) chloride react to form a precipitate.
a) Write a balanced molecular equation for this reaction.
b) Write a balanced complete ionic equation for this reaction.
c) Write a balanced net ionic equation for this reaction.
2. Using a solubility table, decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction.
a) iron(III) nitrate and potassium hydroxide
b) ammonium chloride and lithium carbonate
c) sodium sulfide and nickel(II) sulfate
3. For each of the following equations
i. indicate whether it is a combustion (C), synthesis (S), decomposition (D), single replacement (SR), or double displacement (DD)
ii. indicate which reactions are oxidation-reductions (OR), precipitations (P) or acid-base (AB) reactions.
iii. predict the products and record their formulas. If no reaction occurs, write “NR.” (Use Tables as needed to help you decide if a reaction occurs.)
iv. balance the equation.
a) Li(s) + Cl2(g) ® b) Sr(NO3)2(aq) + K2SO4(aq) ®
c) C3H6(g) + O2(g) ® d) CaCl2(aq) + NaNO3(aq) ®
e) Fe(s) + MgSO4(aq) ® f) KI(l) ®
g) Al(s) + HCl(aq) ® h) HNO3(aq) + KOH(aq) ®
4. Write a chemical equation for the ionization of iron(III) nitrate when it dissolves in water.
5. Chromium reacts with hydrochloric acid in a single replacement reaction. The balanced equation is:
2 Cr(s) + 6 HCl(aq) ® 2 CrCl3(aq) + 3 H2(g)
a) How many moles of HCl are needed to produce 1.60 moles of CrCl3?
b) How many grams of chromium are required to react with 0.450 moles of HCl?
c) How many atoms of chromium are required to produce 12 moles of H2?
d) How many grams of Cr are needed to produce 3.20 g H2?
e) In an experiment, 10.2 grams of CrCl3 are produced starting from 8.30 grams of HCl. What was the theoretical yield and the percent yield in this experiment?
f) When 6.0 moles of Cr are combined with 12.0 moles of HCl, which reactant is limiting? How many moles of excess reactant are left over?
g) How many grams of CrCl3 are produced starting from 13.0 g of Cr and 43.8 g of HCl?
Summary of Chapter 8: Reactions in Aqueous Solutions
predicting whether a reaction will occur
using a solubility table
predicting whether a precipitate occurs
writing equations for precipitation reactions
complete ionic equations
net ionic equations
common strong acids
common strong bases
double displacement reactions
single replacement reactions
Summary of Chapter 9: Chemical Quantities
interpreting balanced chemical equations
mole relationships between reactants and products
mass relationships between reactants and products
calculating percent yield