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| 1 | |
A buffer is prepared by dissolving 4.00 g benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) and 4.00 g sodium benzoate (C6H5COONa) in enough water to prepare 1.00 L of solution. Calculate the pH of this buffer. |
| | A) | 4.13 |
| | B) | 4.20 |
| | C) | 4.27 |
| | D) | 4.40 |
| | E) | 5.05 |
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| 2 | |
Calculate the [NH3]/[NH4+] ratio in an ammonia-ammonium chloride buffer with a pH of 9.00.
(Kb for NH3 = 1.8 x 10-5) |
| | A) | 0.56/1.00 |
| | B) | 0.74/1.00 |
| | C) | 0.86/1.00 |
| | D) | 1.12/1.00 |
| | E) | 1.30/1.00 |
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| 3 | |
A buffer is prepared by adding 0.30 mol CH3COONa to 2.0 L of a 0.10 M CH3COOH solution. Calculate the pH after 0.030 mol HCl are added to the buffer.
(Ka for CH3COOH = 1.8 x 10-5) |
| | A) | 1.52 |
| | B) | 3.57 |
| | C) | 4.81 |
| | D) | 5.13 |
| | E) | 6.34 |
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| 4 | |
What is the pH of a buffer prepared by adding 180 mL of 0.100 M NaOH to 200 mL of 0.100 M acetic acid?
(Ka for CH3COOH = 1.8 x 10-5) |
| | A) | 3.79 |
| | B) | 4.34 |
| | C) | 4.74 |
| | D) | 5.04 |
| | E) | 5.70 |
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| 5 | |
Consider the titration of 50.00 mL of 0.1000 M HBr with 0.1000 M KOH. Calculate the pH after 49.00 mL of the base has been added to the 50.00 mL of HBr. |
| | A) | 2.0 |
| | B) | 3.0 |
| | C) | 4.0 |
| | D) | 6.0 |
| | E) | 7.0 |
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| 6 | |
Calculate the pH at the equivalence point for the titration of 0.20 M aniline (C6H5NH2) with 0.20 M HCl. (Kb for aniline = 3.8 x 10-10) |
| | A) | 2.6 |
| | B) | 2.8 |
| | C) | 5.2 |
| | D) | 9.4 |
| | E) | 11.1 |
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| 7 | |
Citric acid, H3C6H5O7, is a triprotic acid, with Ka1 = 7.5 x 10-4, Ka2 = 1.7 x 10-5, and
Ka3 = 4.0 x 10-7. 1.00 x 10-3 mol of aqueous citric acid is titrated with 0.100 M NaOH. Predict the pH of the titration mixture after the addition of 15.0 mL of the NaOH solution. |
| | A) | 2.68 |
| | B) | 3.12 |
| | C) | 3.95 |
| | D) | 4.77 |
| | E) | 6.40 |
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| 8 | |
An aqueous solution of a weak acid, HA, is titrated with NaOH solution. The pH at the midpoint of the buffer region is 4.5. What is the Ka of the acid? |
| | A) | 3.2 x 10-5 |
| | B) | 3.2 x 10-10 |
| | C) | 1.8 x 10-3 |
| | D) | 7.0 x 10-7 |
| | E) | 4.5 |
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| 9 | |
Which of the following best describes the acid/base properties of normal rainwater, in the absence of any man-made pollutants? |
| | A) | very acidic |
| | B) | slightly acidic |
| | C) | neutral |
| | D) | slightly basic |
| | E) | may be basic or acidic |
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| 10 | |
Given that the solubility of Ag2CrO4 is 0.0287 g/L, what is the value of its Ksp? |
| | A) | Ksp = 3.9 x 10-17 |
| | B) | Ksp = 6.5 x 10-13 |
| | C) | Ksp = 8.7 x 10-5 |
| | D) | Ksp = 7.5 x 10-9 |
| | E) | Ksp = 2.6 x 10-12 |
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| 11 | |
The solubility of AlF3 is 6.7 g AlF3 per liter of solution. What is the value of the solubility product constant for AlF3? |
| | A) | 1.9 x 10-2 |
| | B) | 6.0 x 10-3 |
| | C) | 1.1 x 10-3 |
| | D) | 4.0 x 10-4 |
| | E) | 4.1 x 10-5 |
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| 12 | |
How many grams of AgCl will dissolve in 1.0 L of water? (Ksp for AgCl = 1.7 x 10-10) |
| | A) | 1.2 x 10-12 g |
| | B) | 2.4 x 10-8 g |
| | C) | 4.5 x 10-5 g |
| | D) | 1.8 x 10-3 g |
| | E) | 1.4 x 10-2 g |
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| 13 | |
Calculate the pH of a solution necessary to just begin the precipitation of Mg(OH)2 when
[Mg2+] = 0.001 M. (Ksp for Mg(OH)2 = 1.2 x 10-11) |
| | A) | 11 |
| | B) | 10 |
| | C) | 9 |
| | D) | 8 |
| | E) | 4 |
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| 14 | |
In qualitative analysis, the metals of Ion Group 1 can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and Pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl- concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium?
(Ksp for AgCl = 1.8 x 10-10; Ksp for PbCl2 = 1.7 x 10-5) |
| | A) | [Ag+] = 1.8 x 10-11 M; [Pb2+] = 1.7 x 10-6 M |
| | B) | [Ag+] = 1.8 x 10-7 M; [Pb2+] = 1.7 x 10-4 M |
| | C) | [Ag+] = 1.8 x 10-11 M; [Pb2+] = 8.5 x 10-5 M |
| | D) | [Ag+] = 1.8 x 10-9 M; [Pb2+] = 1.7 x 10-3 M |
| | E) | [Ag+] = 1.8 x 10-9 M; [Pb2+] = 8.5 x 10-6 M |
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| 15 | |
Silver chloride is relatively insoluble in water (Ksp for AgCl = 1.8 x 10-10) but it is soluble in aqueous ammonia, due to the formation of the complex ion Ag(NH3)2+. How many moles of AgCl will dissolve in 1.00 L of solution containing 6.0 moles of free NH3? (Kf for Ag(NH3)2+ = 1.7 x 107) |
| | A) | 9.1 x 10-6 mol |
| | B) | 2.9 x 10-4 mol |
| | C) | 0.0091 mol |
| | D) | 0.084 mol |
| | E) | 0.33 mol |
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