Chapter 16

Chapter 16 - Chapter 16: Acid-Base Equilibria and...

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Page 300 Chapter 16: Acid-Base Equilibria and Solubility Equilibria A table of ionization constants and K a 's is required to work some of the problems in this chapter. 1. In which one of the following solutions will acetic acid have the greatest percent ionization? A) 0.1 M CH 3 COOH B) 0.1 M CH 3 COOH dissolved in 1.0 M HCl C) 0.1 M CH 3 COOH plus 0.1 M CH 3 COONa D) 0.1 M CH 3 COOH plus 0.2 M CH 3 Ans: A Category: Medium Section: 16.2 2. Which one of the following is a buffer solution? A) 0.40 M HCN and 0.10 KCN D) 0.10 M KCN B) 0.20 M CH 3 COOH E) 0.50 M HCl and 0.10 NaCl C) 1.0 M HNO 3 and 1.0 M NaNO 3 Ans: A Category: Medium Section: 16.3 3. Which one of the following combinations cannot function as a buffer solution? A) HCN and KCN D) HF and NaF B) NH 3 and (NH 4 ) 2 SO 4 E) HNO 2 and NaNO 2 C) HNO 3 and NaNO 3 Ans: C Category: Medium Section: 16.3 4. Which of the following is the most acidic solution? A) 0.10 M CH 3 COOH and 0.10 M CH 3 COONa B) 0.10 M CH 3 COOH C) 0.10 M HNO 2 D) 0.10 M HNO 2 and 0.10 M NaNO 2 E) 0.10 M CH 3 COONa Ans: C Category: Medium Section: 16.2 5. Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C 6 H 5 CO 2 H) and 0.15M sodium benzoate (C 6 H 5 COONa). [K a = 6.5 × 10 –5 for benzoic acid] A) 3.97 B) 4.83 C) 4.19 D) 3.40 E) 4.41 Ans: A Category: Medium Section: 16.3 6. A solution is prepared by mixing 500. mL of 0.10 M NaOCl and 500. mL of 0.20 M HOCl. What is the pH of this solution? [K a (HOCl) = 3.2 × 10 –8 ] A) 4.10 B) 7.00 C) 7.19 D) 7.49 E) 7.80 Ans: C Category: Medium Section: 16.3
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Chapter 16: Acid-Base Equilibria and Solubility Equilibria Page 301 7. Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [K a (HCNO) = 2.0 × 10 –4 ] A) 0.97 B) 3.10 C) 4.40 D) 3.70 E) 4.30 Ans: E Category: Medium Section: 16.3 8. Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. a (HOCl) = 3.2 × 10 –8 A) 0.39 B) 3.94 C) 6.58 D) 7.49 E) 8.40 Ans: C Category: Medium Section: 16.3 9. Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [K a (HCNO) = 2.0 × 10 –4 A) 0 B) 3.0 C) 3.7 D) 4.4 E) 5.0 Ans: B Category: Medium Section: 16.3 10. You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 ± 0.02. What molar ratio of CH 3 COOH to CH 3 COONa should be used? A) 0.18 B) 0.84 C) 1.19 D) 5.50 E) 0.10 Ans: D Category: Difficult Section: 16.3 11. What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution? A) H + + H 2 O H 3 O + D) H + + HOCl H 2 OCl + B) H + + OCl HOCl E) HCl + HOCl H 2 O + Cl 2 C) HOCl H + Ans: B Category: Medium Section: 16.3 12. Consider a buffer solution prepared from HOCl and NaOCl. Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?
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This note was uploaded on 02/08/2012 for the course CHEM 161 taught by Professor Shaklovich during the Spring '10 term at Harvard.

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Chapter 16 - Chapter 16: Acid-Base Equilibria and...

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