Honors Chemistry Chapter 4 Review Terms: (know these terms and ...

Honors Chemistry
Chapter 4 Review
Terms: (know these terms and how they relate to each other)
Solvent
Solute
Electrolyte
o Strong / Weak / Non-
Dissociation
Solvation
Chemical Equilibrium
Precipitate
Molecular / Complete Ionic / Net ionic
equations
Soluble
Insoluble
Acid
o Strong / Weak
Base
o Strong / Weak
Ionic salt
Oxidation
Reduction
Concentration
Molarity
Dilution
Titration
Equivalence point
Reaction types:
Precipitation (double replacement)
Neutralization
Single replacement (displacement)
Oxidation-reduction (redox)
Practice problems
1) Which compounds are insoluble in water?
a. Na 2 SO 4
b. PbI 2
c. H 3 PO 4
d. BaCO 3
e. AgNO 3
f. (NH 4 ) 2 S
g. LiOH
2) Label each compound in problem 1 as Acid, Base, or Ionic Compound
3) Write a balanced chemical equation for following double replacement reactions.
a. MgSO 4(aq) + BaCl 2(aq)
b. CaCl 2(aq) + Na 2 CO 3(aq)
c. Lead(ii)nitrate and sodium chloride
d. lithium iodide and calcium phosphate
4) For each reaction in problem 3, write a complete ionic and net ionic equation
5) Identify each compound as a strong or weak acid or base.
a. HClO 3
b. NaOH
c. Mg(OH) 2
d. HNO 2
e. Ca(OH) 2
f. HBr
g. HCN

6) Name each compound in problem 5.
7) Write a balanced chemical equation for the following neutralization reactions.
a. HNO 3(aq) + KOH (aq)
b. HClO 4(aq) + Fe(OH) 2(s)
c. solid chromium(iii)hydroxide and sulfuric acid
d. Aluminum hydroxide and hydrochloric acid
8) What is the oxidation number of the boldfaced element in each compound?
a. NO 2
b. HCO 3
c. CCl 4
d. PbS
e. KMnO 4
9) Using the activity series, write a balanced chemical equation for the following reactions if they take
place.
a. Nickel metal is added to a solution of copper(ii) nitrate
b. a solution of zinc nitrate is added to a solution of magnesium sulfate.
c. Hydrochloric acid is added to gold metal
10) Write a balanced chemical equation for the following reactions (synthesis, decomposition,
combustion, single replacement) and identify which elements have been oxidized and reduced.
a. Br 2(l) + K (s)
b. CH 4(g) + O 2(g)
c. Al (s) + CuCl 2(aq)
11) How many grams of solute are present in 15.0mL of 0.736 M K 2 Cr 2 O 7 ?
12) If 14.00 g of (NH 4 ) 2 SO 4 is dissolved in enough water to form 250 mL of solution, what is the
molarity of the solution?
13) How many milliliters of 0.0455 M CuSO 4 contain 3.65 g of solute?
14) What volume of 0.115M HClO 4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?
15) What volume of 0.128 M HCl is needed to neutralize 2.87g of Mg(OH) 2 ?
16) If 25.8 mL of AgNO 3 is needed to precipitate all the Cl - ions in a 0.785 g sample of KCl(forming
AgCl), what is the molarity of the AgNO 3 solution?
17) If 45.3 mL of 0.108 M HCl solution is needed to neutralize a solution of KOH, how many grams of
KOH must be present in the solution?

ANSWERS
1) Which compounds are insoluble in water?
a. Na 2 SO 4 Soluble Ionic
b. PbI 2 Insoluble Ionic
c. H 3 PO 4 Soluble (it’s an acid) Weak acid
d. BaCO 3 Insoluble Ionic
e. AgNO 3 Soluble Ionic
f. (NH 4 ) 2 SSoluble Ionic
g. LiOH Soluble Strong Base
2) Label each compound in problem 1 as Acid, Base, or Ionic Compound
3) Write a balanced chemical equation for following double replacement reactions.
a. MgSO 4(aq) + BaCl 2(aq) MgCl 2(aq) + BaSO 4(s)
b. CaCl 2(aq) + Na 2 CO 3(aq) CaCO 3(s) + 2NaCl (aq)
c. Lead(ii)nitrate and sodium chloride
Pb(NO 3 ) 2(aq) + 2NaCl (aq) PbCl 2(s) + 2NaNO 3(aq)
d. lithium iodide and calcium phosphate
LiI (aq) + Ca 3( PO 4 ) 2(aq) No Reaction
4) For each reaction in problem 3, write a complete ionic and net ionic equation
a. Mg 2+ (aq) + SO 4
2-
(aq) + Ba 2+ (aq) + 2Cl - (aq)Mg 2+ (aq) 2Cl - (aq) + BaSO 4(s)
i. SO 4
2-
(aq) + Ba 2+ (aq) BaSO 4(s)
b. Ca 2+ (aq) + 2Cl - (aq) + 2Na + (aq) + CO 3
2-
(aq) CaCO 3(s) + 2Na + (aq) + 2Cl - (aq)
i. Ca 2+ (aq) + CO 3
2-
(aq) CaCO 3(s)
c. Pb 2+ (aq) + 2NO 3
-
(aq) + 2Na + (aq) + 2Cl - (aq) PbCl 2(s) + 2Na + (aq) + NO 3
-
(aq)
i. Pb 2+ (aq) + 2Cl - (aq) PbCl 2(s)
d. LiI (aq) + Ca 3( PO 4 ) 2(aq) No Reaction
5) Identify each compound as a strong or weak acid or base.
a. HClO 3 Strong Acid Chloric acid
b. NaOH Strong Base Sodium hydroxide
c. Mg(OH) 2 Weak Base Magnesium hydroxide
d. HNO 2 weak Acid Nitrous acid
e. Ca(OH) 2 Strong Base Calcium hydroxide
f. HBr Strong Acid Hydrobromic acid
g. HCN Weak Acid Hydrocyanic acid
6) Name each compound in problem 5.
7) Write a balanced chemical equation for the following neutralization reactions.
a. HNO 3(aq) + KOH (aq) H 2 O (l) + KNO 3(aq)
b. HClO 4(aq) + Fe(OH) 2(s) H 2 O (l) + Fe(ClO 4 ) 2(aq)
c. Cr(OH) 2(s) + H 2 SO 4(aq) 2H 2 O (l) + CrSO 4(aq)
d. Al(OH) 3(s) + 3HCl (aq) AlCl 3(aq) + 3H 2 O (l)
8) What is the oxidation number of the boldfaced element in each compound?
a. NO 2 +4
d. PbS +2
b. HCO 3 +5
e. KMnO 4 +7
c. CCl 4 +4

9) Using the activity series, write a balanced chemical equation for the following reactions if they take
place.
a. Ni (s) + Cu(NO 3 ) 2(aq) Ni(NO 3 ) 2(aq) + Cu (s)
b. Zn(NO 3 ) 2(aq) + MgSO 4(aq) no reaction
c. Au (s) + HCl (aq) no reaction
10) Write a balanced chemical equation for the following reactions
a. Br 2(l) + 2K (s) 2KBr (s) Oxy: K, Red: Br
b. CH 4(g) + O 2(g) CO 2(g) + H 2 O (g) Oxy:C, Red:O
c. 2Al (s) + 3CuCl 2(aq) 2AlCl 3(aq) + 3Cu (s) Oxy: Al, Red: Cu
11) 3.25 g
12) 0.424 M
13) 503 mL
14) 38.0 mL
15) 769 mL
16) 0.408 M
17) 0.275 g

Polyatomic Ions
+
NH 4
NO 2-
NO 3-
2-
SO 3
2-
SO 4
-
HSO 4
OH -
CN -
3-
PO 4
2-
HPO 4
H2PO 4
-
CO 3
2-
-
HCO 3
ClO -
-
ClO 2
-
ClO 3
-
ClO 4
-
C 2 H 3 O 2
-
MnO 4
2-
Cr 2 O 7
2-
CrO 4
2-
O 2
ammonium
nitrite
nitrate
sulfite
sulfate
hydrogen sulfate
hydroxide
cyanide
phosphate
hydrogen phosphate
dihydrogen phosphate
carbonate
hydrogen carbonate
hypocholorite
chlorite
chlorate
perchlorate
acetate
permanganate
dichromate
chromate
peroxide
Soluble Ionic Compounds
Important Exceptions
Sodium ion, Potassium ion, Ammonium (+) None
Nitrate
None
Acetate
None
Chloride, Bromide, Iodide Compounds of Ag + , Hg 2+ 2 , Pb 2+
Sulfate Compounds of Ba 2+ , Hg 2+ , Pb 2+ , Sr 2+
Insoluble Ionic Compounds
Important exceptions
carbonate, phosphate
Compounds of alkali metal ions, ammonium
Sulfide Compounds of alkali metal ions, ammonium, Ca 2+ ,
Sr 2+ , Ba 2+
Hydroxide Compounds of alkali metal ions, ammonium, Ba 2+ ,
Ca 2+ , Sr 2+