Problem Set #10 – The pH of Solutions of Weak Acids and Bases Refer to Tables 10.1 and 10.2 in your notes for needed K a and K b values. 1. Calculate the pH and pOH of 0.29 M CH 3 COOH(aq) and 0.29 M CCl 3 COOH(aq) and explain any difference on the basis of molecular structure. 2. Calculate the pOH, pH, and percentage protonation of solute in a 0.0073 M solution of codeine, given that the pK a of its conjugate acid is 8.21 3. Determine whether an aqueous solution of each of the following salts has a pH equal to, greater than, or less than 7. If pH <7 or pH >7, write a chemical equation to justify your answer: (a) NH 4 Br; (b) Na 2 CO 3 ; (c) KF; (d) KBr; (e) AlCl 3 ; (f) Cu(NO 3 ) 2 4. Calculate the pH of (a) 0.63 M NaCH 3 CO 2 (aq) and (b) 0.055 M AlCl 3 (aq) 5. (a) When the pH of 0.10 M HClO 2 (aq) was measured, it was found to be 1.2. What are the values of K a and pK a for chlorous acid? (b) When the pH of 0.10 M C 3 H 7 NH 2 (aq) [propylamine] was measured, it was found to be 11.86.
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This note was uploaded on 03/01/2011 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas.