1.
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Since HSO4- is a stronger acid than H2CO3, which of the following statements is true?
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2.
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At 100°C, Kw is about 9 x 10-12. At this temperature, what is the pH of pure water, and is it acidic, basic, or neutral?
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3.
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What is the pH of a solution prepared by dissolving 0.150 g Ca(OH)2 in enough water to have a solution volume of 250.0 mL?
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4.
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What is [H3O+] in a 0.080 M HNO2 solution? For HNO2, Ka = 7.2 x 10-4.
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5.
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Acetic acid has a Ka of 1.8 x 10-5. What is the molarity of an acetic acid solution if it is 1.3% ionized?
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6.
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What is the [PO43-] in a solution that is 0.10 M H3PO4? For H3PO4, Ka1 = 7.1 x 10-3, Ka2 = 6.3 x 10-8, and Ka3 = 4.2 x 10-13.
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7.
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Use appropriate data tables in the appendix of the textbook to determine which of the following salts make acidic solutions when dissolved in water. a. NH4NO2
b. CH3NH3F
c. CH3NH3Cl
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8.
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A typical bleach solution is about 0.070 M NaOCl. For HOCl, Ka = 2.9 x 10-8. What is the pH of this solution?
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9.
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The pH of a solution of NH4C2H3O2 is approximately 7. The best explanation is that
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10.
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Determine the pH of 263 mL of solution that has [NH4I] = 0.300 M. Kb = 1.74 x 10-5 for aqueous NH3.
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