Modified True/False
Indicate
whether the statement is true or false. If false, change the identified word or phrase to make the
statement true.
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1.
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The pH of 0.0050 mol/L solutions of Ca(OH)2 and NaOH are compared.
The NaOH has a higher pH. ______________________________
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2.
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For the gaseous equilibrium shown, 2A + 3B <====> C + 2D + heat.
If the
temperature of the system is decreased, the quantity of B will increase 3/2 as much as
the quantity of A. ______________________________
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3.
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A concentrated weak base can have a lower pOH than a dilute strong base.
_________________________
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4.
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Conjugate acid base partners differ by a single proton.
_________________________
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5.
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Sodium ions have too weak a pull on water's electrons to make
donating protons impossible. _________________________
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Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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6.
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When solid zinc hydroxide is in equilibrium with its ions, the ratio of zinc ion
to hydroxide ion is which of the following?
a. | 1:2 | d. | 1:3 | b. | 2:1 | e. | 2:3 | c. | 1:1 |
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7.
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When solid plumbous sulfate is in equilibrium with its ions, the ratio of
plumbous ion to sulfate ion is which of the following?
a. | 1:2 | d. | 3:1 | b. | 2:1 | e. | 1:3 | c. | 1:1 |
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8.
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When solid barium fluoride is in equilibrium with its ions, the ratio of
fluoride ion to barium ion is which of the following?
a. | 1:1 | d. | 2:3 | b. | 1:2 | e. | 3:2 | c. | 2:1 |
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9.
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In a saturated solution of lead(II) chloride, the concentration of chloride ion
is 6.2 ´ 10-4 mol/L. The Ksp of lead(II) chloride would be
which of the following?
a. | 1.9 ´ 10-7 | d. | 2.3 ´ 10-17 | b. | 6.0 ´
10-11 | e. | none of
the above | c. | 1.2 ´
10-10 |
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10.
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In a saturated solution of aluminum hydroxide, the concentration of aluminum ion
is 2.4 ´ 10-8 mol/L. The Ksp of aluminum hydroxide would
be which of the following?
a. | 1.7 ´ 10-15 | d. | 9.0 ´ 10-30 | b. | 4.2 ´
10-23 | e. | none of
the above | c. | 1.0 ´
10-30 |
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11.
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In a saturated solution of NiCO3, the concentration of nickel(II) ion
is 7.6 ´ 10-4 mol/L. The Ksp of nickel(II) carbonate would
be which of the following?
a. | 5.8 ´ 10-7 | d. | 7.6 ´ 10-4 | b. | 1.2 ´
10-6 | e. | none of the
above | c. | 4.4 ´
10-10 |
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12.
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In a saturated solution of Al(OH)3 the concentration of
OH1- is 2.6 ´ 10-5 mol/L. The concentration of
Al3+ in mol/L is which of the following?
a. | 2.6 ´ 10-5 | d. | 7.8 ´ 10-5 | b. | 5.2 ´
10-5 | e. | 8.7 ´ 10-4 | c. | 7.8 ´
10-15 |
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13.
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For the equilibrium system below, which of the following would result in a
decrease in the quantity of PCl5(g)?
PCl3(g) + Cl2(g)
<=====> PCl5(g) + 45 kJ
a. | increasing temperature | d. | decreasing the size of the container | b. | adding some
Cl2(g) | e. | injecting
some He gas | c. | decreasing temperature |
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14.
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For the equilibrium system below, which of the following would result in an
increase in the quantity of Cl2(g)?
PCl3(g) + Cl2(g)
<=====> PCl5(g) + 45 kJ
a. | adding some PCl3(g) | d. | increasing the volume of the
container | b. | removing some PCl5(g) | e. | injecting some He gas | c. | decreasing
temperature |
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15.
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For the equilibrium system below, which of the following would result in an
increase in the quantity of H2(g)?
H2(g) + I2(g) <=====>
2HI(g) + 65 kJ
a. | removing some I2(g) | d. | both b and c | b. | removing some
HI(g) | e. | both a and
b | c. | decreasing temperature |
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16.
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Some CO2 is removed from the equilibrium system shown below. Which of
the following statements is/are true when the equilibrium responds to this
stress?
CO(NH2)2(g) + H2O(g) + 45 kJ <=====>
CO2(g) + 2 NH3
a. | heat is released as the equilibrium shifts to replace the removed
CO2 | b. | the quantity of NH3 will rise twice as much as
CO2 | c. | the quantity of H2O(g) will rise | d. | both a and b are
true | e. | both b and c are true |
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17.
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10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2
mol of hydrogen gas is found in the container. The number of moles of ammonia gas left in the
container must be which of the following?
N2(g) + 3H2(g) <=====>
2NH3(g) + 94 kJ
a. | 6.8 | d. | 8.8 | b. | 6.4 | e. | 9.2 | c. | 8.6 |
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18.
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10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2
mol of hydrogen gas is found in the container. The Ke for this equilibrium must be which of the
following?
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. | 1.8 ´ 103 | d. | 3.0 | b. | 5.6 ´ 10-4 | e. | 2.8 | c. | 73 |
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19.
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Which of the following systems would be considered to be at equilibrium:
I.
an open flask with 2.0 mL of perfume
II. a closed flask with 10 mL of water
III. an open flask
with 10 mL of water
IV. a closed flask with an ice cube and 10 mL of water
a. | I | d. | II | b. | I and II | e. | III | c. | II and
IV |
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20.
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A full syringe contains this equilibrium
2 NO2(g) <======>
N2O4(g)
If nitrogen dioxide gas is brown and the other gas is colourless,
what is observed when the syringe is used to compress this gas mixture?
a. | the mixture gets darker | d. | the mixture gets
lighter | b. | the mixture gets darker then lighter | e. | none of the above | c. | the mixture get
lighter then darker |
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21.
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If the equilibrium constant for an equilibrium system is decreased by an
increase in temperature then
a. | [reactants] and [products] decreases | b. | [reactants] and [products] increases | c. | [reactants] increases and [products]
decreases | d. | [reactants] decreases and [products]
increases | e. | none of the above |
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22.
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If the equilibrium constant for an equilibrium system is increased by an
increase in temperature then
a. | [reactants] and [products] decreases | b. | [reactants] and [products] increases | c. | [reactants] increases and [products]
decreases | d. | [reactants] decreases and [products]
increases | e. | none of the above |
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23.
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Consider the following system at equilibrium: C 2H 2(g) +
Br 2(g) + 44 kJ <======> C 2HBr 2(g) Which of the following
actions would cause the Ke to increase? I. increasing
the volume at constant pressure and temperature
II. decreasing the volume at constant pressure and
temperature
III. increasing the
temperature
IV. adding bromine gas at
constant temperature and pressure
V.
removing ethyne gas at constant temperature and pressure
VI. decreasing the temperature a. | I and II | d. | III | b. | III and VI | e. | VI | c. | IV and
V |
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24.
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Consider the following system at equilibrium: C 2H 2(g) +
Br 2(g) + 44 kJ <======> C 2H 2Br 2(g) Which of the
following actions would cause the Ke to decrease? I. increasing
the volume at constant pressure and temperature
II. decreasing the volume at constant pressure and
temperature
III. increasing the
temperature
IV. adding bromine gas at
constant temperature and pressure
V.
removing ethyne gas at constant temperature and pressure
VI. decreasing the temperature a. | I and II | d. | III | b. | III and VI | e. | VI | c. | IV and
V |
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25.
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Consider this equilibrium
4HCl(g) + O2(g) <=====>
2H2O(g) + 2Cl2(g)
The equilibrium law expression for the balanced chemical
equation would be
a. | [HCl][O2] /
[H2O][Cl2] | d. | [HCl]4[O2] /
[H2O]2[Cl2]2 | b. | [H2O]2[Cl2]2/
[HCl]4[O2] | e. | [H2O][Cl2]/HCl][O2]
| c. | 2[H2O][Cl2]/
4[HCl][O2] |
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26.
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A precipitate of zinc hydroxide sits at the bottom of a test tube of distilled
water. If the Ksp of this substance is 3.0 ´ 10-16 the
[Zn] in this solution in mol/L is which of the following?
a. | 8.4 ´ 10-6 | d. | 2.4 ´ 10-8 | b. | 4.2 ´
10-6 | e. | 7.5 ´ 10-17 | c. | 1.2 ´
10-8 |
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27.
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The Ksp for a substance A2B is 1.2 ´
10-12. The [B] must be which of the following?
a. | 4.0 ´ 10-11 | d. | 1.3 ´ 10-4 | b. | 3.6 ´
10-12 | e. | 2.6 ´ 10-4 | c. | 6.7 ´
10-5 |
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28.
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The Ksp expression for silver sulfate is Ksp =
a. | [Ag][S] | d. | [Ag]2[SO42-] | b. | [Ag][SO42-] | e. | none of the above | c. | [Ag][SO42-]2 |
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29.
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The Ksp expression for Al(OH)3 is Ksp =
a. | 3[Al][OH1-] | d. | 1/3[Al][OH1-]3 | b. | 3[Al][OH] | e. | [Al][OH1-]3 | c. | 3[Al][OH1-]3 |
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30.
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The Ksp expression for lead(II) bromide is Ksp =
a. | [Pb]2[Br] | d. | [Pb2+]2[Br1-] | b. | [Pb2+][Br2-] | e. | [Pb2+][Br1-]2 | c. | [Pb2+][Br1-] |
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31.
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The Ksp for a substance A2B is 1.2 ´
10-12. The [A] must be which of the following?
a. | 4.0 ´ 10-11 | d. | 1.3 ´ 10-4 | b. | 3.6 ´
10-12 | e. | none of
the above | c. | 6.7 ´ 10-5 |
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32.
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The Ksp for a substance AB3 is 7.8 ´
10-10. The [B] is which of the following?
a. | 7.0 ´ 10-3 | d. | 1.6 ´ 10-2 | b. | 2.3 ´
10-3 | e. | 2.9 ´ 10-11 | c. | 5.3 ´
10-3 |
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33.
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Which of the following salts act like acids when applied to the soil?
a. | BeCl2 | d. | NaF | b. | KF | e. | KCl | c. | FeI3 |
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34.
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Which of the following solutions would not act like acids if added to the
soil?
a. | FeBr3 | d. | PbBr4 | b. | MnCl7 | e. | LiI | c. | CrI6 |
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35.
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If a pH meter was placed in a 1.4 mol/L solution of nitric acid the reading
would be which of the following?
a. | 1.4 | d. | 0.15 | b. | 14.15 | e. | 0.0 | c. | –0.15 |
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36.
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Which of the following salts acts like an acid when added to water?
a. | ammonium nitrate | d. | both a and b | b. | potassium nitrite | e. | both a and c | c. | iron(III)
nitrate |
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37.
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Which of the following salts could be combined with
HC2H3O2 to form a buffer?
a. | sodium oxalate | d. | manganous cyanate | b. | iron(III) gluconate | e. | both c and d | c. | sodium
acetate |
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38.
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Which of the following salts could be combined with
H2C2O4 to make a buffer solution?
a. | ferrous cyanate | d. | sodium hydrogen carbonate | b. | lithium
oxalate | e. | lithium hydrogen
phosphite | c. | potassium hydrogen oxalate |
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39.
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When 45 mL of 0.25 mol/L sulfuric acid is mixed with 25 mL of 0.48 mol/L calcium
hydroxide the solution is/has a
a. | acidic | d. | pH below 7 | b. | neutral | e. | both a and d | c. | basic |
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40.
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When 45 mL of 0.65 mol/L acetic acid is added to 65 mL of 0.45 mol/L sodium
hydroxide the resulting mixture is/has a(n)
a. | neutral | d. | pH < 7 | b. | basic | e. | both c and d | c. | acidic |
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41.
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When the solids hydrated Ba(OH)2 and NH4SCN are mixed they
dissolve in the water of hydration and the temperature drops significantly. This system has which of
the following?
a. | increased entropy and decreased enthalpy | b. | decreased entropy
and increased enthalpy | c. | increased both entropy and
enthalpy | d. | decreased both entropy and enthalpy | e. | none of the
above |
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42.
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For this chemical system
KOH(s) + HBr(aq) ®
KBr(aq) + H2O(l) + 45 kJ
which of the following is true?
a. | entropy has increased and enthalpy has decreased | b. | entropy has
decreased and enthalpy has increased | c. | both entropy and enthalpy have
decreased | d. | both entropy and enthalpy have increased | e. | heat of
neutralization = 45 kJ/mol of HBr |
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43.
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The Ka for four acids are
H2CO3 – 4.5 ´ 10–7, HCO2H – 1.8 ´ 10-4, H3C6H5O7-
7.1 ´ 10-4, HCN – 6.2 ´ 10-10. If the pH's of 0.50 mol/L solutions of these acids
were measured and they were placed in order from highest pH to lowest pH the results would be which
of the following?
a. | HCN, H3C6H5O7, HCO2H,
H2CO3 | d. | H3C6H5O7,
HCO2H, H2CO3, HCN | b. | H2CO3, HCN,
H3C6H5O7, HCO2H | e. | HCN, H2CO3,
H3C6H5O7, HCO2H | c. | HCN,
H2CO3, HCO2H,
H3C6H5O7 |
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44.
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If sodium monohydrogen phosphite was dissolved in distilled water, which of the
following could be added to make a functional buffer?
a. | potassium dihydrogen phosphate | d. | phosphoric acid | b. | potassium dihydrogen
phosphite | e. | sodium dihydrogen
phosphate | c. | phosphorous acid |
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45.
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Kw is which of the following?
a. | the equilibrium constant for water which is always 1.0 ´ 10-14 | b. | Ka ´ Kb for
conjugate acid - base partners @ 25oC | c. | the log[H2O] @
25oC | d. | both a and c | e. | none of the
above |
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46.
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For phosphoric acid, H3PO4, the Ka1 =
a. | [PO43-][H1+]3 /
[H3PO4] | d. | [H3PO4] /
[H2PO41-][H1+] | b. | [HPO42-][H1+] /
[H3PO4] | e. | [H3PO4] /
[PO43-][H1+]3 | c. | [H2PO41-][H1+] /
[H3PO4] |
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47.
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For sulfurous acid the Ka1 =
a. | [SO32-][H1+]2 /
[H2SO3] | d. | [HSO31-][H1+] /
[H2SO3] | b. | [HSO42-][H1+] /
[H2SO3] | e. | [H2SO3] /
[SO31-][H1+]2 | c. | [SO31-][H1+]2 /
[H2SO3] |
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48.
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For cyanide ion (CN1-) the Kb =
a. | [OH1-][HCN] /
[CN1-] | d. | [C4-][N3+] /
[CN1-] | b. | [CN1-] /
[OH1-][HCN] | e. | none of the above | c. | [OH1-][HCN1-] /
[CN] |
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49.
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A solution of sodium oxalate has a pH of 7.82. The [OH1-]
in mol/L must be which of the following?
a. | 6.18 | d. | 7.82 | b. | 1.5 ´
10-8 | e. | –7.82 | c. | 6.6 ´
10-7 |
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50.
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If the Kb of a weak acid is 2.9 ´
10-8, the Ka of its conjugate acid partner must be which of the following?
a. | 2.9 ´ 10-8 | d. | 3.1 ´ 10-7 | b. | 6.46 | e. | 3.4 ´
10-7 | c. | 7.54 |
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Completion
Complete each
statement.
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51.
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If solutions of barium chloride and sodium sulfate were mixed and a precipitate
formed, the precipitate would be _________________________.
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52.
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If solutions of strontium chloride and potassium chromate were mixed and a
precipitate formed, the precipitate would be ______________________________.
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53.
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If solutions of lead(II) nitrate and lithium chloride were mixed and a
precipitate formed, the precipitate would be _________________________.
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54.
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If solutions of aluminum fluoride and potassium hydroxide were mixed and a
precipitate formed, the precipitate would be ______________________________.
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55.
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If solutions of calcium fluoride and potassium carbonate were mixed and a
precipitate formed, the precipitate would be ______________________________.
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56.
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If solutions of sodium phosphate and zinc bromide were mixed and a precipitate
formed, the precipitate would be _________________________.
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57.
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If solutions of silver nitrate and potassium cyanide were mixed and a
precipitate formed, the precipitate would be _________________________.
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58.
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If solutions of lithium sulfite and barium iodide were mixed and a precipitate
formed, the precipitate would be _________________________.
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59.
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If solutions of barium chloride and sodium sulfate were mixed and a precipitate
formed, the equilibrium equation for the precipitate would be
_____________________________________________.
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60.
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If solutions of copper(II) nitrate and sodium carbonate were mixed and a
precipitate formed, the equilibrium equation for the precipitate would be
_____________________________________________.
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61.
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If solutions of iron(II) chloride and potassium phosphate were mixed and a
precipitate formed, the equilibrium equation for the precipitate would be
_____________________________________________.
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62.
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When solid magnesium carbonate is in equilibrium with its ions, the ratio of
magnesium ion to carbonate ion is ____________________.
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63.
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When solid barium monohydrogen phosphate is in equilibrium with its ions, the
ratio of barium ion to monohydrogen phosphate ion is ____________________.
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64.
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CO(g) + 2H2(g) ® CH3OH(l);
during this reaction the entropy ____________________.
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65.
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S(s) + 2N2O(g) ® SO2(g) +
2N2(g); during this reaction the entropy ____________________.
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66.
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NH3(g) + HCl(g) ®
NH4Cl(s); during this chemical change the algebraic sign for the entropy change is
predicted to be ____________________.
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67.
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4NO(g) ® 2N2O(g) + O2(g);
during this chemical change the algebraic sign for the entropy change is predicted to be
____________________.
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68.
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A system at equilibrium always has forward and reverse reactions which are
___________________________________.
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69.
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A solution at 25oC with a pOH of 3.45 has a pH of
____________________.
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70.
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The [H1+] of a 0.95 mol/L solution of HBr at
25oC is ____________________.
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71.
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When potassium hydroxide is titrated to an end point by sulfuric acid the salt
formed is _________________________.
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72.
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When nitric acid is titrated to an end point by lithium hydroxide the salt
formed is _________________________.
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73.
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When iron(III) hydroxide is combined with carbonic acid the salt formed is
_________________________.
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Matching
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Here is a list of weak acids. Match to its conjugate base partner below. If
no match exists indicate by writing none. a. | H2O | d. | HPO42- | b. | HSO41- | e. | H2CO3 | c. | HC2H3O2 | f. | H2C6H6O6 |
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74.
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OH1-
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75.
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HCO31-
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Each of the numbers below represent [H1+] ions in
solution. Match these to the correct [OH1-] in the same solution. All numbers
are in mol/L. a. | 3.4 ´
10-3 | c. | 9.8 ´ 10-8 | b. | 2.4 ´ 10-5 | d. | 1.7 ´ 10-4 |
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76.
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5.9 ´ 10-11
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Short Answer
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77.
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Consider the equilibrium below:
If 1.2 mol of HI was placed in a
1.0 L container and allowed to reach equilibrium what would the value of Ke be if at equilibrium
[HI] = 0.40 mol/L.
H2(g) + I2(g) <=====> 2HI(g)
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78.
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Write an equilibrium expression showing how the fluoride ion acts like a base.
Be sure to identify the conjugate acid-base partners in the equilibrium.
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79.
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If the [OH1-] of a solution at 25oC is 7.7 ´ 10-12 mol/L, calculate the [H1+] in
mol/L, the pH, and the pOH.
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80.
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Write the Kb expression for the weak base
NO2-1(aq).
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81.
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Write the equilibrium expression for the self ionization of NH3.
Assume it follows the same pattern as water.
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Problem
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82.
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If the solubility of CaF2 is 2.3 ´ 10-4
mol/L, what is its Ksp?
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83.
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If the solubility of Al(OH)3 is 3.2 ´ 10-09
mol/L, what is its Ksp?
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84.
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If the concentration of Ba2+ is
found to be 4.2 ´
10-8 mol/L in a saturated solution of this salt,
what is the Ksp of Ba3(PO4)2?
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85.
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If 1.7 L of a saturated solution of AgC2H3O2 is found to contain 14.1 g of AgC2H3O2, what is the Ksp of AgC2H3O2.
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86.
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If 1.4 L of a saturated solution of Ag2CO3 is found to
contain 0.049g of Ag2CO3, what is the Ksp of
Ag2CO3.
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87.
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What is the solubility, in mol/L, of CaF2 in a 0.65 mol/L solution of
NaF, if the Ksp of CaF2 is 4.9 ´ 10-11?
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88.
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What is the concentration of a monoprotic weak acid if its pH is 5.50 and its
Ka = 5.7 ´ 10-10?
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89.
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What is the percent ionization of a 1.38 mol/L weak acid if its Ka =
2.7 ´ 10-6?
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90.
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A weak acid with a concentration of 0.53 mol/L has a percent ionization of
0.062%. What is the pH of this weak acid?
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91.
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25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35 mol/L
acetic acid. Calculate the pH of the solution.
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92.
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28 mL of 0.36 mol/L acetic acid is titrated with a standardized 0.43 mol/L KOH
solution. Calculate the pH of the solution after 21 mL of the KOH solution has been added. Assume the
Ka of acetic acid is 1.8 ´ 10-5.
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Essay
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93.
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Acid rain is a serious environmental problem. Given the equations for a variety
of chemical reactions which contribute to this problem, discuss how human activity adds to the
overall load of acidic substances. Make sure to include in your discussion strong and weak acids and
include equilibrium expressions for one weak acid. Also discuss how the oxides of sulfur and nitrogen
are formed through combustion and describe how these oxides react with water forming strong and weak
acids. Suggest some measures which would reduce the problem.
N2(g) +
O2(g) <====>2NO(g)
2NO(g) + O2(g) ------->
2NO2(g)
SO2(g) + H2O(g) ------>
H2SO3(aq)
2NO2(g) + H2O(g)----->HNO3(aq)
+ HNO2(aq)
SO3(g) + H2O ------->
H2SO4(aq)
S(s) + O2(g) ------->
SO2(g)
2SO2(g) + O2(g) -------> 2SO3(g)
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94.
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Impurities of sulfur in coal, natural gas and gasoline create environmental
problems. Limestone is an abundant natural resource which contains CaCO3. Use these
equations to discuss how the rain is becoming increasing acidified and suggest potential solutions to
our acid rain problems.
N2(g) + O2(g) <====>2NO(g)
2NO(g) +
O2(g) -------> 2NO2(g)
SO2(g) + H2O(g)
------> H2SO3(aq)
2NO2(g) +
H2O(g)----->HNO3(aq) +
HNO2(aq)
SO3(g) + H2O ------->
H2SO4(aq)
S(s) + O2(g) ------->
SO2(g)
2SO2(g) + O2(g) ------->
2SO3(g)
CaCO3(s) + SO2(g) -----> CaSO3(g) +
CO2(g)
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