Calculate the pH of the solution obtained by titrating 500mL of

# Calculate the ph of the solution obtained by

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7. [McQuarrie 21-38] Calculate the pH of the solution obtained by titrating 50.0mL of 0.100M HNO 2 (aq) with 0.150M NaOH(aq) to the equivalence point. Take K a = 5 . 4 · 10 - 4 for HNO 2 (aq). 8. [McQuarrie 21-42] Calculate the pH for each of the following cases in the titration of 35.0mL of 0.200M methylamine, CH 3 NH 2 (aq), with 0.200M HCl(aq). K b, CH 3 NH 2 = 4 . 6 · 10 - 4 . (a) before addition of any HCl(aq) (b) after addition of 17.5mL of HCl(aq) (c) after addition of 34.9mL of HCl(aq) (d) after addition of 35.0mL of HCl(aq) (e) after addition of 35.1mL of HCl(aq)
9. [McQuarrie 21-47] What is required to form a buffer solution? Can a buffer solution resist a change in pH due to the addition of acid or base indefinitely? 10. [McQuarrie 21-49] Under what conditions can we apply the Hendersen-Hasselbalch equation to determine the pH of a buffer solution? 11. [McQuarrie 21-54] Why is the pH at the equivalence point for the titration of a strong acid with a strong base equal to 7.00, but generally not equal to 7.00 for the titration of a weak acid with a strong base? 12. [McQuarrie 21-57] You are given a sample of a solid unknown monoprotic weak acid. Describe how you could usea titration curve to determine both the molecular mass and the value of pK a of the unknown acid. Would this be sufficient information to positively identify the unknown acid?

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