Chemistry
Mr. Reger
Review Guide – Ch. 7 – Answers
Name ________________________
Date _____________ Period _____
Non-accelerated students may use the solubility rules on p.172 of your textbook.
1. Are the following salts soluble or insoluble in water? Give an explanation for each.
a) MgCO3
insoluble (carbonate salts are insoluble)
b) SrCl2
soluble (most halide salts are soluble)
c) Pb(NO3)2
soluble (nitrate salts are soluble)
d) Na3PO4
soluble (Group 1 salts are soluble)
e) BaSO4
insoluble (most sulfates are soluble; BaSO4, CaSO4, and PbSO4 are exceptions)
f) (NH4)2CO3 soluble (ammonium salts are soluble)
g) PbBr2
insoluble (most halide salts are soluble; PbBr2 is an exception)
2. Identify each compound as an acid, a base, or neither. Name each compound.
Acid/Base/Neither
Name
a) H2CO3
acid
carbonic acid
b) K2Cr2O7
neither
potassium dichromate
c) Ca(OH)2
base
calcium hydroxide
d) CH3COOH
acid
acetic acid
e) HBr
acid
hydrobromic acid
f) RbOH
base
rubidium hydroxide
g) HNO3
acid
nitric acid
h) HNO2
acid
nitrous acid
i) CuSO4
neither
copper(II) sulfate
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3. Predict the products of each reaction, write the balanced molecular equation (including
symbols for the physical state), and give the name of each product. Then write complete ionic
and net ionic equations for each reaction.
a) Aqueous sodium carbonate + aqueous barium nitrate  sodium nitrate + barium carbonate
Molecular equation:
Na2CO3(aq) + Ba(NO3)2(aq)  2 NaNO3(aq) + BaCO3(s)
Complete ionic equation:
2 Na+(aq) + CO32-(aq) + Ba2+(aq) + 2 NO3-(aq)  2 Na+(aq) + 2 NO3-(aq) + BaCO3(s)
Net Ionic equation:
CO32-(aq) + Ba2+(aq)  BaCO3(s)
b) Aqueous sulfuric acid + aqueous lead(II) acetate  lead(II) sulfate + acetic acid
Molecular equation:
H2SO4(aq) + Pb(CH3COO)2(aq)  PbSO4(s) + 2 CH3COOH(aq)
Complete ionic equation:
2 H+(aq) + SO42-(aq) + Pb2+(aq) + 2 CH3COO-(aq)  PbSO4(s) + 2 CH3COO-(aq) + 2 H+(aq)
Net Ionic equation:
SO42-(aq) + Pb2+(aq)  PbSO4(s)
c) Aqueous nitric acid + aqueous potassium hydroxide  potassium nitrate + water
Molecular equation:
HNO3(aq) + KOH(aq)  KNO3(aq) + H2O(l)
Complete ionic equation:
H+(aq) + NO3-(aq) + K+(aq) + OH-(aq)  K+(aq) + NO3-(aq) + H2O(l)
Net Ionic equation:
H+(aq) + OH-(aq)  H2O(l)
d) Aqueous iron(III) nitrate + aqueous beryllium chlorideberyllium nitrate + iron(III) chloride
Molecular equation:
2 Fe(NO3)3(aq) + 3 BeCl2(aq)  3 Be(NO3)2(aq) + 2 FeCl3(aq)
Complete ionic equation:
2 Fe3+(aq) + 6 NO3-(aq) + 3 Be2+(aq) + 6 Cl-(aq)  3 Be2+(aq) + 6 NO3-(aq) + 2 Fe3+(aq) + 6 Cl-(aq)
Net Ionic equation:
No Reaction !!
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4. Balance each reaction. Then classify each reaction in as many ways as possible.
a) 2 Al(s) + 3 ZnCl2(aq)  3 Zn(s) + 2 AlCl3(aq)
redox, single replacement
b) KClO4(s)  KCl(s) + 2 O2(g)
decomposition
c) 2 HNO3(aq) + Mg(OH)2(aq)  Mg(NO3)2(aq) + 2 H2O (l)
acid-base, double displacement
d) Hg(l) + Cl2(g)  HgCl2(s)
synthesis, redox
e) 2 Na(s) + 2 H2O(l)  2 NaOH(aq) + H2(g)
single replacement, redox
f) 2 C2H6(g) + 7 O2(g)  4 CO2(g) + 6 H2O(l)
combustion, redox
g) Ba(OH)2(aq) + H2SO4(aq)  2 H2O(l) + BaSO4(s)
acid-base, precipitation, double displacement
h) 3 Ca(s) + N2(g)  Ca3N2(s)
synthesis, redox
i) Fe(NO3)2(aq) + Rb2CO3(aq)  FeCO3(s) + 2 RbNO3(aq)
precipitation, double displacement
j) CuSO4(s)  CuO(s) + SO3(g)
decomposition
k) 2 Mg(s) + O2(g)  2 MgO(s)
combustion, synthesis, redox
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5. For each redox reaction below, indicate which species is oxidized and which is reduced.
a) 2 Mg(s) + O2(g)  2 MgO(s)
Mg is oxidized; O is reduced
b) Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)
Zn is oxidized; H is reduced
c) 3 I2(s) +2 Al(s)  2 AlI3(s)
Al is oxidized; I is reduced
d) 2 AgNO3(aq) + Cu(s)  Cu(NO3)2(aq) + 2 Ag(s)
Ag is reduced; Cu is oxidized
e) Zn(s) + H2SO4(aq)  ZnSO4(aq) + H2(g)
Zn is oxidized; H is reduced
6. Write a balanced net ionic equation for each reaction.
a) CH3COOH(aq) + Mg(OH)2(s) 
2 H+(aq) + Mg(OH)2(s)  2 H2O(l) + Mg2+(aq)
b) (NH4)2CO3(aq) + SrCl2(aq) 
CO32-(aq) + Sr2+(aq)  SrCO3(s)
c) Cs2SO4(aq) + Ca(NO3)2(aq) 
SO42-(aq) + Ca2+(aq)  CaSO4(s)
d) Ba(OH)2(aq) + H2SO4(aq) 
Ba2+(aq) + 2 OH-(aq) + 2 H+(aq) + SO42-(aq)  BaSO4(s) + 2 H2O(l)
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