Exam 980415
Name___________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) Will a precipitate be observed if 0.10 mol Ag
+
and 0.001 mol SO42- are added to make 1.0 L of solution? ( Ksp = 1.4 × 10-5)A) Yes, because Q > Ksp.
B) No, because Q > Ksp.
C) Yes, because Q < Ksp.
D) No, because Q < Ksp.
E) More information is needed to answer this question.
Answer: D
2) At 25.0°C the enthalpy of vaporization of water ( Hvap) is 44.0 kJ/mol and the vapor pressure is 23.8 mm Hg. Calculate the vapor pressure of water at 50.0°C, in mm Hg.
A) 6.02 B) 147 C) 58.2 D) 564 E) 94.1
Answer: E
3) Which of the following describes what happens to the solubility of a slightly soluble ionic compound when a common ion is added to the solution?
A) More of the ionic compound dissolves.
B) The solubility of the ionic compound is increased.
C) There is no effect on the solubility of the ionic compound.
D) The solubility of the ionic compound is reduced.
E) The ionic compound dissolves more rapidly.
Answer: D
4) A saturated solution of AB2 contains 8.60 x 10-4 moles AB2 per liter. Determine Ksp.
A) 6.36 x 10-10 B) 7.40 x 10-7 C) 1.27 x 10-9 D) 1.48 x 10-6 E) 2.54 x 10-9 Answer: E
5) In the plot of ln(k) versus 1/T for a first order reaction, the frequency factor (A) can be determined by A) the negative of the slope of the line times R.
B) the intercept of the x-axis.
C) the slope of the line times R.
D) the slope of the line.
E) the intercept on the y-axis.
Answer: E
6) The vapor pressure of acetone is 400. mm Hg at 25°C, and Hvap = 32.0 kJ/mol. What is the temperature
7) Given the values of G° shown below, determine the value of G° for the reaction.
3 A + 1 B 3 C + 2 D
G° (J/mol K) 261 97.0 181 122
A) 101 B) -93.0 C) 93.0 D) -55.0 E) 1670
Answer: B
8) At 50°C, the solubility of silver chloride, AgCl, is 5.2 x 10-4 g/100 mL. Calculate the Ksp at this temperature.
A) 7.6 × 108 B) 1.8 × 10-10 C) 4.0 × 10-5 D) 1.0 × 10-8 E) 1.3 × 10-9 Answer: E
9) Which of the following mixtures/solutions would be a buffer solution?
A) 25 mL 1 M NaOH + 50 mL 1 M CH3COOH B) 25 mL 1 M NaOH + 50 mL 1 M NH3 C) 50 mL 1 M HCl + 50 mL 1 M NH3 D) 50 mL 1 M HCl + 50 mL 1 M NaOH
E) none of these Answer: A
10) Refer to the information in Figure 1. What is the predicted rate law for Mechanism II?
Two mechanisms proposed for the following reaction of nitrogen dioxide with carbon monoxide are shown below. Use this information to answer the following questions.
NO2 (g) + CO CO2 (g) + NO (g)
Mechanism I: NO2 (g) + CO CO2 (g) + NO (g) (one step) Mechanism II: NO2 (g) + NO2 (g) NO3 (g) + NO (g) (slow) NO3 (g) + CO (g) CO2 (g) + NO2 (g) (fast)
Figure 1 A) rate = k[NO2]
B) rate = k[NO2] 2 C) rate = k[NO2] 2[CO]
D) rate = k[NO2][CO]
E) rate = k[NO3][CO]
Answer: B
11) The addition of large quantities of C2O42- to a solution of Ca2+ causes:
Ca2+ (aq) + C2O42- (aq) CaC2O4 (s) A) precipitation of CaC2O4.
B) Ksp to increase.
C) an increase in [Ca2+].
D) precipitation of Ca2+.
E) Ksp to decrease.
Answer: A
12) Which process is accompanied by a decrease in entropy for the system?
A) water evaporates B) ethanol condenses C) dry ice sublimes D) wax melts
E) sodium chloride dissolves Answer: B
13) In the titration of 20.0 mL of 0.200 M HOBr with 0.100 M NaOH, what is the pH at the equivalence point?
(Ka HOBr = 2.5 × 10-9)
A) 10.86 B) 7.00 C) 4.40 D) 3.29 E) 10.71
Answer: E
14) At 300 K, for equilibrium in the reaction A + B C + D, H = +500 kJ, and Kp = 1 × 10-10. Which of the following statements is incorrect?
A) The reaction is endothermic.
B) G° > 0 C) G° = 0
D) The equilibrium favors the reactants.
E) G = 0 Answer: C
15) What is the pKa if the Ka is 0.00000860 ?
A) 5.1 B) -5.1 C) 4.8 D) 10 E) 5.4
Answer: A
16) What is the molar solubility for a slightly soluble salt whose Ksp = 2.0 × 10-16 ? A2B2 (s) 2 A
+
(aq) + 2 B
-
(aq)
A) 2.3 x 10-6 B) 3.5 x 10-9 C) 1.7 x 10-4 D) 5.9 x 10-5 E) 1.2 x 10-4 Answer: D
17) Above what temperature, in °C, will the following reaction become spontaneous? Assume free energy, enthalpy, and entropy are not temperature dependent.
18) Which of the following reactions leads to an increase in entropy of the system?
A) CaO (s) + CO2 (g) CaCO3 (s) B) 4 Fe (s) + 3 O2(g) 2 Fe2O3 (s) C) NH4Cl (s) HCl (g) + NH3 (g) D) 2 HI (g) + Cl2 (g) 2 HCl (g) + I2 (s)
E) CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (l) Answer: C
19) What is the pH of a solution containing 0.00044 moles H+ per liter?
A) 3.7 B) -3.4 C) 3.4 D) 0.00044 E) 1.0
Answer: C
20) If 100. mL of 0.025 M NaCl is mixed with 150. mL of 0.0015 M Pb(NO3)2, will a precipitate form?
(Ksp PbCl2 = 1.6 × 10-5) A) No, because Qip > Ksp.
B) Yes, because Qip > Ksp.
C) Yes, because Qip < Ksp.
D) No, becauseQip < Ksp.
E) No, because Qip = Ksp.
Answer: D
21) Identify the Lewis Base in the following equation.
H+ + NH3 NH4+
A) H2O B) H+
C) NH3 D) NH4+
E) not an acid-base reaction Answer: C
22) The pH of acid rain may be as low as 2.80. What is the H3O
+
in such acidic rain?A) 1.6 B) 630 C) 6.3 × 10-12 D) 1.6 × 10-3 E) 9.7 × 10-2
Answer: D
23) Which of the following salts is most soluble in pure water?
A) ZnS, Ksp = 1.6 × 10-24 B) CuS, Ksp = 8.7 × 10-36 C) PbI2, Ksp = 7.1 × 10-9 D) HgS, Ksp = 2.0 × 10-53
E) AgI, Ksp = 8.5 × 10-17 Answer: C
24) The conjugate acid of HPO42- is A) H2PO4
-
B) PO43- C) H3PO4 D) H2PO42-
E) none of these Answer: A
25) What conditions would apply to a reaction that is not spontaneous at low temperature but becomes spontaneous at higher temperatures?
A) decrease in enthalpy and increase in entropy B) increase in enthalpy and decrease in entropy C) decrease in enthalpy and decrease in entropy D) increase in enthalpy and increase in entropy
E) No conditions allow for such a result.
Answer: D
26) A saturated solution of Mg(OH)2 has a pH of 11.03. Determine the Ksp for Mg(OH)2.
A) 4.96 × 10-12 B) 6.1 × 10-10 C) 1.15 × 10-8 D) 6.1 × 10-8 E) 6.2 × 10-12 Answer: B
27) Calculate the molar concentration of free Ag+ in an aqueous solution that is 0.20 M AgNO3 and also 2.5 M Na2S2O3. (Kf [Ag(S2O3)2]3- = 1.7 × 1013)
A) 1.5 × 1013 B) 2.7 × 10-15 C) 2.5 × 10-5 D) 1.9 × 10-15 E) 4.7 × 10-15 Answer: B
28) Calculate the pH after 10.0 mL of 0.40 M NaOH is added to 20.0 mL of 0.50 M HCl.
A) 0.30 B) 7.00 C) 13.30 D) 0.70 E) 13.70
Answer: D
29) Which of the following is the strongest acid?
A) HCl B) H2S C) PH3 D) SiH4 E) CH4
Answer: A
30) What is the correct Ksp expression for Ca3(PO4)2?
A) [Ca2+] [PO43-]
B) [Ca2+]3 [PO]4 C) [Ca3+] [PO42-]
D) [Ca2+]3 [P]2 [O4]2 E) [Ca2+]3 [PO43-]2 Answer: E
31) For which of the following processes would the entropy change be positive?
A) I2 (s) I2 (aq)
32) Calculate the pOH of a 3.5 × 10-2 M NaOH solution.
A) 1.46 B) 12.54 C) 0.46 D) 2.46 E) 11.46
Answer: A
33) For a certain reaction, the standard free energy change is -80.0 kJ at 300 K and -40.0 kJ at 600 K. For this reaction
A) H is positive, and S is positive.
B) H is positive, and S is negative.
C) H is negative, and S is negative.
D) H is negative, and S is positive.
E) impossible to tell Answer: C
34) In the titration of 20.0 mL of 0.200 M HOBr with 0.100 M NaOH, what is the pH after 20.0 mL of the NaOH solution is added? (Ka HOBr = 2.5 × 10-9)
A) 8.60 B) 4.65 C) 5.74 D) 7.00
E) none of these Answer: A
35) The solubility product for Zn(OH)2 is 3.0 × 10-16. What is the molar concentration of Zn2+ ions in a solution of pH = 9.00 ?
A) 3.0 × 10-6 B) 6.8 × 10-6 C) 300 D) 4.2 × 10-6 E) 7.5 × 10-7
Answer: A
36) Which of the following variables are NOT needed to solve the van't Hoff equation?
A) temperature B) enthalpy
C) universal gas constant D) equilibrium constant
E) entropy Answer: E
37) What is the value of Ka for an acid if [H3O+] = 0.13 M, [A-] = 0.820 M, and [HA] = 2.00 M at equilibrium ?
A) 0.48 B) 0.54 C) 19 D) 0.053 E) 0.21
Answer: D
38) Given the following Ka values,
HC2H3O2 1.8 × 10-5 HClO3 5.0 × 102
HCN 6.2 × 10-10 HF 6.6 × 10-4
HOCl 2.9 × 10-8 which of the following is the weakest base?
A) ClO3- B) F- C) OCl- D) CN- E) C2H3O2-
Answer: A
39) Consider the following exothermic reaction:
N2 (g) + 3 H2 (g) 2 NH3 (g)
Which of the following changes would not increase the amount of NH3 produced from given quantities of N2 and H2?
A) an increase in T B) a decrease in V
C) removing some NH3 and reestablishing equilibrium D) an increase in P
E) none of the above Answer: A
40) Which one of the following processes is not spontaneous and endothermic (at 1 atm)?
A) melting of ice at 10°C B) sublimation of CO2 at 25°C C) H2O (l) H2O (g) at 101°C
D) dissolving the soluble salt, NH4NO3, and the temperature drops E) condensation of water at 99°C
Answer: E
41) The metal center in a complex ion is A) a Lewis acid.
B) a ligand.
C) a Lewis base.
D) a Bronsted-Lowry base.
E) insoluble in the solvent.
Answer: A
42) For the phase transition from solid to liquid, Hfusion = 15.1 kJ/mol and Sfusion = 487 J/mol K. At what temperature ( °C )does this phase transition take place?
A) -273 B) -205 C) -242 D) 0.0310 E) 31.0
Answer: C
43) With which of the following bases will the reaction of acetic acid, CH3COOH, proceed farthest toward completion.
A) Cl- B) NO3- C) CO3-2 D) HSO4- E) F-
Answer: C
44) Calcium sulfate is sometimes added to wine both to clarify and to precipitate dissolved lead. Given the following Ksp values, what [Pb2+] remains in wine that is saturated with CaSO4?
(Ksp CaSO4 = 9.1 × 10-6, Ksp PbSO4 = 1.6 × 10-8)
A) 1.3 × 10-4 B) 1.8 × 10-2 C) 5.3 × 10-6 D) 1.5 × 10-13 E) 3.0 × 10-3 Answer: C
45) What is [H3O+], if the pH = 10 ? A) 1.00 x 10-10
B) 4.54 x 10-5 C) -2.30 D) -1.00
E) 1.00 x 1010 Answer: A
46) Identify the Lewis Acid in the following equation.
AlCl3 + H2O H2OAlCl3
A) H2O B) H+ C) H2OAlCl3 D) AlCl3 E) Cl-
Answer: D
47) Given the following data, what is the value of Gf° (in kJ) for CH3OH (l) at 25°C.
CO2 (g) + 2 H2 (g) CH3OH (l) Keq = 1.081 × 10-40
Gf° kJ/mol -394.4 0 ?
A) -166.4 B) 622.4 C) 92.0 D) 228.0
E) Not enough information is given.
Answer: A
48) A saturated solution of AgCrO3 contains 14 mg AgCrO3 per liter of solution. What is Ksp for AgCrO3?
A) 4.5 × 10-9 B) 2.2 × 108 C) 1.4 × 10-3 D) 1.3 × 10-4 E) 6.7 × 10-5 Answer: A
49) Use Trouton's rule to estimate the normal boiling point of hexane, in °C, given that at this temperature Hvap = 29.8 kJ/mol.
A) 2.9 B) 343 C) 45 D) 34 E) 70
Answer: E
50) In which of the following solutions would the solubility of calcium carbonate be the smallest?
A) pure water
B) 0.5 M sodium chloride C) 0.1 M calcium chloride D) 0.2 M sodium carbonate
E) 0.1 M HCl Answer: D
