Chapter 04 – Reactions in Aqueous Solutions
82. Which of the following represents a hydrogen displacement reaction?
83. Which of the following represents a combustion reaction?
Chapter 04 – Reactions in Aqueous Solutions
84. What type of reaction is the following?
Ca(OH)2(s) + 2 HNO3(aq) → Ca(NO3)2(aq) + 2 H2O(l)
85. What type of reaction is the following?
C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(g)
Chapter 04 – Reactions in Aqueous Solutions
86. The reaction below can be classified as which type of reaction ?
2 NO2(g) + H2O(l) → HNO2(aq) + HNO3(aq)
87. What mass of C6H12O6 (glucose) is needed to prepare 450. mL of a 0.650 M solution of
glucose in water?
Chapter 04 – Reactions in Aqueous Solutions
88. What mass of C12H22O11 (sucrose) is needed to prepare 255 mL of a 0.570 M solution of
sucrose in water?
89. What mass of K2CO3 is needed to prepare 200. mL of a solution having a potassium ion
concentration of 0.150 M?
Chapter 04 – Reactions in Aqueous Solutions
90. What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion
concentration of 0.125 M?
91. What mass of Li3PO4 is needed to prepare 500. mL of a solution having a lithium ion
concentration of 0.175 M?
Chapter 04 – Reactions in Aqueous Solutions
92. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0
mL. What is the ammonium nitrate concentration in the resulting solution?
93. A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added
until the volume of the solution reaches 250. mL. What is the concentration of nitric acid in
the final solution?
Chapter 04 – Reactions in Aqueous Solutions
94. A 3.682 g sample of KClO3 is dissolved in enough water to give 375. mL of solution.
What is the chlorate ion concentration in this solution?
95. A 4.691 g sample of MgCl2 is dissolved in enough water to give 750. mL of solution.
What is the magnesium ion concentration in this solution?
Chapter 04 – Reactions in Aqueous Solutions
96. A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500. mL of solution.
What is the calcium ion concentration in this solution?
97.
35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the concentration of nitrate ion in the
final solution?
Chapter 04 – Reactions in Aqueous Solutions
98. 17.5 mL of a 0.1050 M Na2CO3 solution is added to 46.0 mL of 0.1250 M NaCl. What is
the concentration of sodium ion in the final solution?
99. 25.0 mL of a 0.2450 M NH4Cl solution is added to 55.5 mL of 0.1655 M FeCl3. What is
the concentration of chloride ion in the final solution?
Chapter 04 – Reactions in Aqueous Solutions
100. A 350. mL solution of 0.150 M HNO3(aq) is mixed with a solution of 230. mL of 0.240
M HCl(aq). How many moles of H+(aq) are present in the final solution?
101. A 430. mL solution of 0.230 M HBr(aq) is mixed with a solution of 225 mL of 0.350 M
HClO4(aq). How many moles of H+(aq) are present in the final solution?
Chapter 04 – Reactions in Aqueous Solutions
102. A 110. mL solution of 0.340 M HCl(aq) is mixed with a solution of 330. mL of 0.150 M
HNO3(aq). The solution is then diluted to a final volume of 1.00 L. How many moles of H+
are present in the final solution?
103. When 38.0 mL of 0.1250 M H2SO4 is added to 100. mL of a solution of PbI2, a
precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed.
If the recovered PbSO4 is found to have a mass of 0.0471 g, what was the concentration of
iodide ions in the original solution?
Chapter 04 – Reactions in Aqueous Solutions
104. When 50.0 mL of a 0.3000 M AgNO3 solution is added to 50.0 mL of a solution of
MgCl2, an AgCl precipitate forms immediately. The precipitate is then filtered from the
solution, dried, and weighed. If the recovered AgCl is found to have a mass of 0.1183 g, what
was the concentration of magnesium ions in the original MgCl2 solution?
105. When 20.0 mL of a 0.250 M (NH4)2S solution is added to 150.0 mL of a solution of
Cu(NO3)2, a CuS precipitate forms. The precipitate is then filtered from the solution, dried,
and weighed. If the recovered CuS is found to have a mass of 0.3491 g, what was the
concentration of copper ions in the original Cu(NO3)2 solution?
Chapter 04 – Reactions in Aqueous Solutions
106. 34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H2SO4 solution.
What is the concentration of the original sulfuric acid solution?
107. What volume (mL) of a 0.3428 M HCl(aq) solution is required to completely neutralize
23.55 mL of a 0.2350 M Ba(OH)2(aq) solution?
Chapter 04 – Reactions in Aqueous Solutions
108. What volume (mL) of a 0.2450 M KOH(aq) solution is required to completely neutralize
55.25 mL of a 0.5440 M H3PO4(aq) solution?
109.
The concentration of oxalate ion (C2O42–) in a sample can be determined by titration with a solution of permanganate ion
(MnO4–) of known concentration. The net ionic equation for this reaction is
2MnO4– + 5C2O42– + 16H+ → 2Mn2+ + 8H2O + 10CO2
A 30.00 mL sample of an oxalate solution is found to react completely with 21.93 mL of a 0.1725 M solution of MnO4–.
What is the oxalate ion concentration in the sample?
Chapter 04 – Reactions in Aqueous Solutions
110. One method of determining the concentration of hydrogen peroxide (H2O2) in a solution
is through titration with the iodide ion. The net ionic equation for this reaction is
H2O2 + 2I– +2H+ → I2 + 2H2O
A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with 37.12
mL of a 0.1500 M KI solution. What is the concentration of hydrogen peroxide in the
sample?
111. Zinc dissolves in hydrochloric acid to yield hydrogen gas:
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
What mass of hydrogen gas is produced when a 7.35 g chunk of zinc dissolves in 500. mL of
Chapter 04 – Reactions in Aqueous Solutions
112. Zinc dissolves in hydrochloric acid to yield hydrogen gas:
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
When a 12.7 g chunk of zinc dissolves in 500. mL of 1.450M HCl, what is the concentration
of hydrogen ions remaining in the final solution?
113. Lithium metal dissolves in water to yield hydrogen gas and aqueous lithium hydroxide.
What is the final concentration of hydroxide ions when 5.500 g of lithium metal is dropped
into 750. mL of water?
Chapter 04 – Reactions in Aqueous Solutions
114. When solid iron(II) hydroxide is added to water, the resulting solution contains 1.410–
3g of dissolved iron(II) hydroxide per liter of solution. What is the hydroxide ion
concentration in this solution?
115. A 250. mL sample of 0.0328M HCl is partially neutralized by the addition of 100. mL of
0.0245M NaOH. Find the concentration of hydrochloric acid in the resulting solution.
Chapter 04 – Reactions in Aqueous Solutions
116. A 350. mL sample of 0.276M HNO3 is partially neutralized by 125 mL of 0.0120M
Ca(OH)2. Find the concentration of nitric acid in the resulting solution.
117. 158 mL of a 0.148M NaCl solution is added to 228 mL of a 0.369M NH4NO3 solution.
The concentration of ammonium ions in the resulting mixture is
Chapter 04 – Reactions in Aqueous Solutions
118. 1.40 g of silver nitrate is dissolved in 125 mL of water. To this solution 5.00 mL of
1.50M hydrochloric acid is added, and a precipitate forms. Find the concentration of silver
ions remaining in solution.
119. Select True or False: A solution is a homogeneous mixture of two or more substances.
120. Select True or False: Al(NO3)3 is a strong electrolyte.
Chapter 04 – Reactions in Aqueous Solutions
121. Select True or False: NH4NO3 is a weak electrolyte.
122. Select True or False: H3PO4 is a weak electrolyte.
123. Select True or false: H2CO3is a weak electrolyte.