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CHM-152 > Test 3 > Flashcards

Test 3 Flashcards

1
Q

A titration of an acid and base to the equivalence point results in a noticeably acidic solution. It is likely this titration involves
A) a weak acid and a strong base.
B) a strong acid and a weak base
C) a strong acid and a strong base.
D) a weak base and a weak acid.
E) a weak acid and a weak base (where Ka equals Kb).

A

B) a strong acid and a weak base

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2
Q 
2. For which type of titration will the pH be neutral at the equivalence point?
A) Weak acid vs. strong base. 
B) Strong acid vs. weak base. 
C) Strong acid vs. strong base.
D) All of the above.
E) None of the above.
A

C) Strong acid vs. strong base.

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3
Q 
3. For which type of titration will the pH be basic at the equivalence point?
A) Strong acid vs. strong base. 
B) Strong acid vs. weak base. 
C) Weak acid vs. strong base.
D) All of the above.
E) None of the above.
A

C) Weak acid vs. strong base.

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4
Q 
4. .Which one of the following is a buffer solution?
A) 0.40 M HCN and 0.10 KCN 
B) 0.20 M CH3COOH 
C) 1.0 M HNO3 and 1.0 M NaNO3
D) 0.10 M KCN
E) 0.50 M HCl and 0.10 NaCl
A

0.40 M HCN and 0.10 KCN

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5
Q 
Identify the conjugate base of HSO4 –
A) OH– 
B) H2SO4 
C) H2O
D) H2SO3 
E) SO42–
A

E) SO42–

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6
Q 
Identify the conjugate acid of HCO3–
A) H2O 
B) CO32– 
C) H2CO3 
D) CO2 
E) H3O+
A

C) H2CO3

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7
Q 
The OH– concentration in a 7.5 × 10–3 M Ca(OH)2 solution is
A) 7.5 × 10–3 M. 
B) 1.5 × 10–2 M.
C) 1.3 × 10–12 M.
D) 1.0 × 10–7 M.
E) 1.0 × 10–14 M
A

B) 1.5 × 10–2 M.

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8
Q 
Calculate the H+ ion concentration in a 8.8 × 10–4 M Ca(OH)2 solution.
A) 8.8 × 10–4 M 
B) 1.8 × 10–3 M 
C) 2.2 × 10–11 M
D) 1.1 × 10–11 M
E) 5.7 × 10–12 M
A

E) 5.7 × 10–12 M

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9
Q 
Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.
A) 1.00 
B) 0.00070 
C) 3.15 
D) 5.15 
E) 7.00
A

D) 5.15

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10
Q 
Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.
A) HOCl < HClO3 < HClO2 
B) HOCl < HClO2 < HClO3 
C) HClO2 < HOCl < HClO3
D) HClO3 < HOCl < HClO2
E) HClO3 < HClO2 < HOCl
A

B) HOCl < HClO2 < HClO3

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11
Q

When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength?
A) bond strength
B) electron withdrawing effects
C) percent ionic character of the H–X bond
D) solubility
E) Le Châtelier’s principle

A

A) bond strength

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12
Q 
Which of these species will act as a Lewis acid?
A) NH3 
B) NH4+ 
C) H2O 
D) BF3 
E) F–
A

D) BF3

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13
Q 
What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x 10-10)
A) 0.96 
B) 10.84 
C) 5.42 
D) 9.89 
E) 4.11
A

C) 5.42

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14
Q 
In which one of the following solutions will acetic acid have the greatest percent ionization?
A) 0.1 M CH3COOH
B) 0.1 M CH3COOH dissolved in 0.1 M HCl
C) 0.1 M CH3COOH dissolved in 0.2 M HCl
D) 0.1 M CH3COOH plus 0.1 M CH3COONa
E) 0.1 M CH3COOH plus 0.2 M CH3COONa
A

A) 0.1 M CH3COOH

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15
Q

Research with biochemical systems commonly requires buffers because ________
A) that’s just the way it is.
B) proteins have a critical pH dependence in their structure and function.
C) proteins decompose into constituent amino acids outside a certain pH range.
D) proteins are buffers.
E) salts are involved.

A

B) proteins have a critical pH dependence in their structure and function.

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16
Q 
What is the pH of a buffer solution where [HA] = [A-]?
A) pH = 1
B) pH = Ka
C) pH = pKa
D) pH = pOH
E) pH = 7.0
A

C) pH = pKa

17
Q 
The pKa of a weak acid was determined to be 3.39 by measuring the pH of a solution containing the weak acid at 0.20 M and its conjugate base. The measured pH was 3.27. What was the concentration of the conjugate base?
A) 0.26 M
B) 0.15 M
C) 0.20 M
D) 0.050 M
E) 0.35 M
A

B) 0.15 M

18
Q 
How many moles of sodium acetate must be added to 500 mL of 0.25 M acetic acid solution to produce a buffer with a pH of 4.94? The pKa of acetic acid is 4.74. You can neglect the change in volume when sodium acetate dissolves in the acetic acid solution.
A) 0.011 moles
B) 0.021 moles
C) 0.125 moles
D) 0.198 moles
E) 0.206 moles
A

D) 0.198 moles

19
Q

In a titration of monoprotic acids and bases, there is a large change in pH ________
A) at the point where pH = pKa of the acid.
B) when the volume of acid is exactly equal to the volume of base.
C) when the concentration of acid is exactly equal to the concentration of base.
D) when the number of moles of acid is exactly equal to the number of moles of base.
E) at the point where pH = pKb of the base.

A

D) when the number of moles of acid is exactly equal to the number of moles of base.

20
Q 
A Lewis base is any species capable of \_\_\_\_\_\_\_\_ an electron pair.
A) accepting
B) donating
C) creating
D) neutralizing
E) gaining
A

B) donating

21
Q 
Calculate the solubility of MgF2 in water if the Ksp for the compound is 6.40 x  10^-9.
A) 2.13 x 10^-9 M
B) 1.86 x 10^-3 M
C) 1.17 x 10^-3 M
D) 1.47 x 10^-3 M
E) 3.25 x 10^-5 M
A

C) 1.17 x 10^-3 M

22
Q 
Lead pipes were used at one time for delivering drinking water. What is the maximum possible concentration of lead in this water if it comes from lead(II) hydroxide (Ksp = 2.8 x 10^-16) dissolving from the surface of the pipes?
A) 4.1 x 10^-6 M
B) 1.6 x 10^-8 M
C) 6.5 x 10^-6 M
D) 5.1 x 10^-6 M
E) 8.3 x 10^-9 M
A

A) 4.1 x 10^-6 M

23
Q

What would happen to the Ag+ and Cl- concentrations if NaCl(s) were dissolved in a saturated solution of AgCl in water?
A) [Ag+] and [Cl-] both would increase.
B) [Ag+] and [Cl-] both would decrease.
C) [Ag+] would become larger, and [Cl-] would become smaller.
D) [Ag+] would become smaller, and [Cl-] would become larger.
E). [Ag+] and [Cl-] would remain the same because the solution is saturated.

A

D) [Ag+] would become smaller, and [Cl-] would become larger.

24
Q 
Which of the following would decrease the Ksp for PbI2?
A) Lowering the pH of the solution 
B) Adding a solution of Pb(NO3)2
C) Adding a solution of KI 
D) None of the above
A

D) None of the above

25
Q 
As the pH decreases, the solubility of \_\_\_\_\_\_\_\_ would increase.
A) lead(II) chloride
B) silver(I) iodate
C) calcium carbonate
D) mercury(I) bromide
E) silver(I) chloride
A

C) calcium carbonate

26
Q 
As the pH increases, the solubility of \_\_\_\_\_\_\_\_ would increase.
A) lead(II) hydroxide
B) barium chloride
C) sodium hydroxide
D) magnesium sulfide
E) aluminum chloride
A

E) aluminum chloride

27
Q 
What is the percent ionization of a 1.5 M HC2H3O2 solution (Ka = 1.8 × 10^–5 ) at 25°C?
A) 0.52 % 
B) 0.35 % 
C) 2.5 % 
D) 0.18 % 
E) 0.28 %
A

A) 0.52 %

28
Q 
A 0.20 M solution of a weak monoprotic acid is 0.22 % ionized. What is the acid-ionization constant, Ka, for this acid?
A) 1.9 x 10-6 
B) 2.2 x 10-6 
C) 1.1 × 10–4 
D) 2.4 x 10–4 
E) 9.7 x 10-7
A

E) 9.7 x 10-7

29
Q 
A 0.10 M aqueous solution of a weak acid HA has a pH of 5.00. What is the value of Ka for HA?
A) 1.0 × 10–8 
B) 1.0 × 10–6 
C) 1.0 x 10-7
D) 1.0 x 10-9 
E) 1.0 x 10-5
A

D) 1.0 x 10-9

30
Q

Suppose 50.00 mL of 2.0 × 10–6 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10–4 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10–14.
A) A precipitate forms because Qc > Ksp.
B) A precipitate forms because Qc < Ksp.
C) No precipitate forms because Qc < Ksp.
D) No precipitate forms because Qc = Ksp.
E) No precipitate forms because Qc > Ksp.

A

C) No precipitate forms because Qc < Ksp.

31
Q

To 1.0L of water, 1.5 x 10-6 mol of Pb(NO3)2, 6.5 × 10–6 mol of K2CrO4 and 1.0 mol of NaCl are added. What will happen ? (Ksp for PbCrO4= 1.8 × 10–14 and Ksp for PbCl2 = l.6 × 10–5
A) A precipitate of KCl will form.
B) A precipitate of PbCrO4 will form.
C) A precipitate of PbCl2 will form.
D) No precipitate will form.
E) Both a Precipitate of PbCl2 and a Precipitate of PbCrO4 will form.

A

B) A precipitate of PbCrO4 will form.

32
Q 
Will a precipitate of Silver Chloride (Ksp (AgCl) = 1.6 x 10–10) form when 400mL of 1.1 x 10-5 M of AgNO3 are added to 600. mL of 1.2 × 10–5 M of NaCl.
A) Yes, Q > Ksp 
B) Yes, Q < Ksp 
C) No, Q < Ksp
D) No, C)Q = Ksp 
E) Yes, Q = Ksp
A

C) No, Q < Ksp

33
Q 
33. If 370 mL of 1 × 10–8 M Al(NO3)3 is mixed with 370 mL of 1 × 10–8 M NaOH, what will occur? For Al(OH)3, Ksp = 4.6 × 10–33.
A) Aluminum hydroxide will precipitate.
B) Sodium hydroxide will precipitate.
C) Aluminum nitrate will precipitate.
D) Sodium nitrate will precipitate.
E) No precipitate will form.
A

E) No precipitate will form.

34
Q 
What is the value of the dissociation constant, Kd, for the complex ion Zn(NH3)42+? For Zn(NH3)42+, Kf = 2.9 × 109.
A) 2.9 × 10^–5. 
B) 7.3 × 10^8 
C) 2.9 × 10^9
D) 2.3 × 10^2 
E) 3.4 × 10^–10
A

E) 3.4 × 10^–10

CHM-152 (3 decks)

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