1. Calculate the pH of a solution that is 0.20 M in NaCH 3 COO and 0.10 M in CH 3 COOH. 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.4.63 2.4.74 3.4.95 4.5.05 5.5.22

2. Calculate the pH of a solution that is 0.12 M in HOCl and 0.20 M in NaOCl. 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.6.76 2.6.32 3.7.24 4.7.68 5.7.76

3. Calculate the pH of 100. mL of 0.100 M acetic acid, CH 3 COOH, to which 0.040 mol of sodium acetate, NaCH 3 COO, has been added. 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.5.87 2.5.35 3.4.62 4.4.99 5.6.26

4. Which of the following combinations is not buffer solution? All components are present in 0.10 M concentrations. 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.HCN and NaCN 2.NH 3 and NH 4 Cl 3.HCl and NH 4 Cl 4.CH 3 COOH and NH 4 CH 3 COO 5.NH 3 and NH 4 CH 3 COO

5. What is the pH of a solution that is 0.20 M in HOCl and 0.15 M NaOCl after 0.050 mol HCl/L has been bubbled into the solution? 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.7.85 2.6.15 3.6.95 4.7.06 5.7.45

6. The nonionized form of an acid indicator is yellow, and its anion is blue. The Ka of this indicator is 10 -5. What will be the approximate pH range over which this indicator changes color? 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.3-5 2.4-6 3.5-7 4.8-10 5.9-11

7. Calculate the pH of the solution resulting from the addition of 40.0 mL of 0.200 M HClO 4 to 60.0 mL of 0.150 M NaOH. 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.1.47 2.2.00 3.11.88 4.12.00 5.13.06

8. Which titration curve could describe the titration of a solution of HCl by addition of a solution of KOH? 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.2. 3. 4.5.

9. Consider the titration of a solution of a weak acid by adding a solution of a strong base. Which response includes all the following statements that are true, and no others? I. The end-point cannot be detected using an indicator. II. The pH at the equivalence point is 7.00. III. The solution is buffered before the equivalence point. IV. The solution is buffered both before and after the equivalence point. V. Methyl orange (pH color range 3.1-4.4) would be a better indicator for this titration than would thymol blue (pH range 8.0-9.6). 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.II and IV 2.III 3.IV and V 4.I and III 5.IV and V

10. What is the pH of the solution resulting from the addition of 20.0 mL of 0.0100 M NaOH solution to 30.0 mL of 0.0100 M acetic acid, CH 3 COOH? 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.2. 3. 4.5.

11. Which titration curve could describe the titration of a solution of NH 3 by addition of a solution of HCl? 1234567891011121314151617181920 2122232425262728293031323334353637383940 41424344454647484950 1.2. 3. 4.5.