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# pb 14 - 7 Calculate the pH of the solution resulting when...

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Problem Set #14 Buffers and Titrations 1. Calculate the pH of a buffer solution that is 0.15 M HNO 2 (aq) and 0.20 M NaNO 2 (aq). 2. Suppose that 0.0200 mol NaOH(s) is dissolved in 300. mL of a buffer solution that is 0.040 M NaCH 3 CO 2 (aq) and 0.080 M CH 3 COOH(aq) at 25 degrees Celsius. Calculate the pH of the resulting solution. 3. Which of the buffer systems in Table 11.1 in the text would be a good choice to prepare a buffer with pH = 5 1? 4. Calculate the ratio of the molarities of acetate ions and acetic acid needed to buffer a solution at pH = 5.25. The pK a of CH 3 COOH is 4.75. 5. Consider a titration of 25.00 mL of 0.250 M NaOH(aq) with 0.340 M HCl(aq). What is the pH of the solution that results from the addition of 10.00 mL of the HCl(aq) titrant to the analyte? 6. Calculate the pH at the stoichiometric point of the titration of 25.00 mL of 0.010 M HClO(aq) with 0.020 M KOH(Aq). K a for HClO is 3.0 x 10 -8
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Unformatted text preview: . 7. Calculate the pH of the solution resulting when 10.00 mL of 0.150 M NaOH(aq) is added to 25.00 mL of 0.100 M HCOOH(aq). Use K a = 1.8 x 10-4 for HCOOH. 8. Calculate the pH at the stoichiometric point of the titration of 25.00 mL of 0.020 M NH 3 (aq) with 0.015 M HCl(aq). (For NH 4 + , K a = 5.6 x 10-10 ) 9. Calculate the ratio of the molarities of benzoate ions and benzoic acid (C 6 H 5 COOH) needed to buffer a solution at pH = 3.50. The pK a of C 6 H 5 COOH is 4.19. 10. Which of the buffer systems listed in Table 11.1 in the text would be a good choice to prepare a buffer with pH = 10 1? 11. Suppose that 0.0100 mol HCl(g) is dissolved in 500. mL of a buffer solution that is 0.040 M NaCH 3 CO 2 (aq) and 0.080 M CH 3 COOH(aq) at 25 degrees Celsius. Calculate the pH of the resulting solution. 12. Calculate the pH of a buffer solution that is 0.040 M NH 4 Cl(aq) and 0.030 M NH 3 (aq)...
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