A certain weak acid, HA, has a Ka value of 9.9x10^-7 1. Calculate the percent di

Question

A certain weak acid, HA, has a Ka value of 9.9x10^-7
1. Calculate the percent dissociation of HA in a 0.10 M solution
2. Calculate the percent dissociation of HA in a 0.010 M solution

Explanation / Answer

HA + H2O -> H3O + A for a 0.10 M solution: Where x is the change in concentration: Ka = [H3O] [A] / [HA] 9.9x10^-7 = x^2 / (0.10 - x) x = 3.14 * 10^-4 mol/L percent dissociation = x / 0.1 * 100 = 3.14 * 10^-1 percent for a 0.010 M solution: Ka = [H3O] [A] / [HA] 9.9x10^-7 = x^2 / (0.010 - x) x = 1.0 * 10^-5 mol/L percent dissociation = x / 0.1 * 100 = 1.0 * 10^-2 percent

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