Question

Calculate the [H+] of the following solutions from their pH. Then, calculate experimental Ka and Kb values using an ICE table.

A. Acetic acid - pH=3.02

B. Ammonuim hydroxide - pH=10.53

Answer #1

A. **[H ^{+}]** = 10

**The experimental Ka value =
[H ^{+}][CH_{3}COO^{-}]/[CH_{3}COOH]**

i.e. **Ka =** **9.55*10 ^{-4} *
9.55*10^{-4}/[CH_{3}COOH]**

**Kb = 10 ^{-14}/Ka**

**Note: [CH _{3}COOH] should be given. If it is
there, you can substitute and calculate accordingly.**

B. **[H ^{+}]** = 10

**The experimental Kb value =
[NH _{4}^{+}][OH^{-}]/[NH_{4}OH]**

i.e. **Ka =** **2.95*10 ^{-11} *
2.95*10^{-11}/[NH_{4}OH]**

**Ka = 10 ^{-14}/Kb**

**Note: [NH _{4}OH] should be given. If it is
there, you can substitute and calculate accordingly.**

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