1. A 1.31 M solution of a weak acid HA is found to have a pH...

Question

Question

1. A 1.31 M solution of a weak acid HA is found to have a pH of 2.09. Determine K, of the acid Determine K of its conjugate b

Answer 1

Answer #1

1. pH = 2.09

So, [H+ ] = 10 - 2.09 (M) = 8.13 * 10-3 M

Ka = [H+]2 / [HA] = (8.13 * 10-3 ) 2 / 1.31 = 5.04 * 10-5

2. Kb = 10 - 14 / Ka = 10-14 / 5.04 * 10-5 = 1.98 * 10-10

3. [OH-] = (2.00 * Kb) 1/2 = (2.00 * 1.98 * 10-10 )1/2 = 1.99 * 10-5 M

4. pOH = - log[OH-] = - log(1.99 * 10-5 ) = 4.70

pH = 14 - pOH = 14 - 4.70 = 9.30

Answer 2

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