Honors Chemistry
Name: __________________________________ Date: ___________________ Mods: ___________
Chapter 4 Review: Aqueous Reactions
1) What do we call the insoluble product formed in a double replacement reaction?
2) When an aqueous ionic compound dissociates, what is meant by this term? What has
happened to the compound?
3) What do we call the ions that appear in identical forms among both the reactants and products
of a complete ionic equation which do not directly participate in the chemical reaction?
4) What are the seven strong acids, by name and chemical formula?
1. _________________________________________ = _________________
2. _________________________________________ = _________________
3. _________________________________________ = _________________
4. _________________________________________ = _________________
5. _________________________________________ = _________________
6. _________________________________________ = _________________
7. _________________________________________ = _________________
5) What is the difference between oxidation and reduction?
6) Given the two examples below, identify which reaction is showing oxidation occurring and
which reaction is showing reduction occurring.
Pt2+ (aq) + 2e–  Pt (s)
=
____________________________
Al (s)  Al3+ (aq) + 3e–
=
_____________________________
7) Describe the relationship between how reactive a metal is and its location on the activity
series. How does this relate to oxidation of a metal?
8) What does it mean to be a noble metal?
9) Classify the following as either an soluble (aq) or insoluble (s):
a.
_______ Li3PO4
e.
_______ CuCO3
i.
_______ CaS
b.
_______ Mg(OH)2
f.
_______ NH4OH
j.
_______ K2SO4
c.
_______ CoCl2
g.
_______ PbBr2
d.
_______ HNO3
h.
_______ AgNO3
10) Fill in the following table based on compound type, solubility, and electrolytic properties:
Compound
PbCO3
Ca(OH)2
AgI
C8H18 (l)
HCl
KClO4
H3PO4
Mg3(PO4)2
NH4Br
HC2H3O2 (aq)
Ionic, Covalent, Acid,
or Base?
Soluble or Insoluble?
Strong, Weak, or
Nonelectrolyte?
11) Single & Double Replacement Reactions: Identify the reactions below as either single
replacement (SR) or double replacement (DR) along the left hand side.

For single replacement rxns: Use the activity series to determine if the reaction will occur. If
it will not occur, write NR for no reaction. If the reaction does occur, predict the products
(including states of matter) and balance the equation.

For double replacement rxns: Predict the products and determine the states of matter using
the solubility table. If both products are aqueous, write NR (signifies that no true chemical
reaction has occurred). If a solid precipitates is formed, a chemical reaction has occurred and
the equation also must be balanced.
SR/DR
______ 1) _____Zn (s) + _____Ca(NO3)2 (aq) 
______ 2) _____HCl (aq) + _____Ag2SO4 (aq) 
______ 3) _____ Cr(C2H3O2)3 (aq) + _____Na (s) 
______ 4) _____Pb(NO3)2 (aq) + _____AlCl3 (aq) 
______ 5) _____Br2 (g) + _____MnI2 (aq) 
______ 6) _____(NH4)2SO4 (aq) + _____HCl (aq) 
______ 7) _____Na2SO4 (aq) + _____BaBr2 (aq) 
______ 8) _____Fe (s) + _____Ag2SO4 (aq) 
______ 9) _____Fe(NO3)2 (aq) + _____H3PO4 (aq) 
12) The following reactions will all occur. For each reaction, predict the products and balance the
molecular equations and write the complete and net ionic equations. [NOTE: These could be
SINGLE or DOUBLE replacement reactions, so determine the type of reaction first. For
complete ionic equations, ONLY AQUEOUS reactants are products are broken up into their
ions, all other states of matter remain together.]
a. Aqueous solutions of lithium hydroxide and tin (II) nitrate are combined.
Balanced Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
b. Potassium metal is placed into a beaker containing phosphoric acid.
Balanced Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation:
c. Aqueous solutions of chromium (III) sulfate and sodium carbonate are combined.
Balanced Molecular Equation:
Complete Ionic Equation:
Net Ionic Equation: