Mastering Chemistry 8
According to the following reaction, what mass of PbCl2 can form from 235 mL of
0.110 M KCl solution? Assume that there is excess Pb(NO3)2.
2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
7.19 g
1.80 g
3.59 g
5.94 g
1.30 g - ANS - 3.59 g
\Based on the balanced chemical equation shown below, determine the molarity
of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required
to completely react with 30.00 mL of a 0.125 M potassium bromate, KBrO3(aq),
solution. The net ionic equation for the reaction is
6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l).
0.562 M
0.0938 M
0.0156 M
1.00 M - ANS - 0.562 M
\Choose the statement below that is FALSE.
A molecular compound does not ionize in solution.
A strong acid solution consists of only partially ionized acid molecules.
Strong electrolytes completely dissociate into ions in water.
Nonelectrolyte solutions do not conduct electricity.
A weak acid solution consists of mostly nonionized acid molecules. - ANS - A
strong acid solution consists of only partially ionized acid molecules
\Define a spectator ion.
an ion in a reaction that has a positive charge.
an ion that does not participate in a reaction.
an ion that participates in a reaction.
an ion in a reaction that has a negative charge. - ANS - an ion that does not
participate in a reaction
, \Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200
M NaCl to 250.0 mL.
0.160 M
0.00800 M
0.0320 M
1.25 M
0.0160 M - ANS - 0.0160 M
\Determine the oxidation state of Sn in Sn(SO4)2.
+4
0
+6
-2
+2 - ANS - +4
\Explain the difference between a strong and weak electrolyte. Give an example of
each.
-A weak electrolyte is only slightly soluble and does not ionize to any great extent
in water; for example, AgCl.
-A weak electrolyte is either an ionic compound that is soluble in water, or a
molecular compound that ionizes completely in water; for example, NaCl.
-A strong electrolyte is only slightly soluble and does not ionize to any great
extent in water; for example, C2H3O2.
-A strong electrolyte is either an ionic compound that is soluble in water, or a
molecular compound that ionizes completely in water; for example, HCl.
-None of the above. - ANS - -A weak electrolyte is only slightly soluble and does
not ionize to any great extent in water; for example, AgCl.
-A strong electrolyte is either an ionic compound that is soluble in water, or a
molecular compound that ionizes completely in water; for example, HCl.
\Give the complete ionic equation for the reaction (if any) that occurs when
aqueous solutions of K2CO3 and HBr are mixed.
- 2 K+(aq) + CO32-(aq) + 2 H+(aq) + 2 Br-(aq) → H2O(l) + CO2(g) + 2 K+(aq) + 2
Br-(aq)
According to the following reaction, what mass of PbCl2 can form from 235 mL of
0.110 M KCl solution? Assume that there is excess Pb(NO3)2.
2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
7.19 g
1.80 g
3.59 g
5.94 g
1.30 g - ANS - 3.59 g
\Based on the balanced chemical equation shown below, determine the molarity
of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required
to completely react with 30.00 mL of a 0.125 M potassium bromate, KBrO3(aq),
solution. The net ionic equation for the reaction is
6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l).
0.562 M
0.0938 M
0.0156 M
1.00 M - ANS - 0.562 M
\Choose the statement below that is FALSE.
A molecular compound does not ionize in solution.
A strong acid solution consists of only partially ionized acid molecules.
Strong electrolytes completely dissociate into ions in water.
Nonelectrolyte solutions do not conduct electricity.
A weak acid solution consists of mostly nonionized acid molecules. - ANS - A
strong acid solution consists of only partially ionized acid molecules
\Define a spectator ion.
an ion in a reaction that has a positive charge.
an ion that does not participate in a reaction.
an ion that participates in a reaction.
an ion in a reaction that has a negative charge. - ANS - an ion that does not
participate in a reaction
, \Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200
M NaCl to 250.0 mL.
0.160 M
0.00800 M
0.0320 M
1.25 M
0.0160 M - ANS - 0.0160 M
\Determine the oxidation state of Sn in Sn(SO4)2.
+4
0
+6
-2
+2 - ANS - +4
\Explain the difference between a strong and weak electrolyte. Give an example of
each.
-A weak electrolyte is only slightly soluble and does not ionize to any great extent
in water; for example, AgCl.
-A weak electrolyte is either an ionic compound that is soluble in water, or a
molecular compound that ionizes completely in water; for example, NaCl.
-A strong electrolyte is only slightly soluble and does not ionize to any great
extent in water; for example, C2H3O2.
-A strong electrolyte is either an ionic compound that is soluble in water, or a
molecular compound that ionizes completely in water; for example, HCl.
-None of the above. - ANS - -A weak electrolyte is only slightly soluble and does
not ionize to any great extent in water; for example, AgCl.
-A strong electrolyte is either an ionic compound that is soluble in water, or a
molecular compound that ionizes completely in water; for example, HCl.
\Give the complete ionic equation for the reaction (if any) that occurs when
aqueous solutions of K2CO3 and HBr are mixed.
- 2 K+(aq) + CO32-(aq) + 2 H+(aq) + 2 Br-(aq) → H2O(l) + CO2(g) + 2 K+(aq) + 2
Br-(aq)
