Problem: The Ka of a monoprotic weak acid is 8.15 × 10-3. What is the percent ionization of a 0.146 M solution of this acid?

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Recall: The percent ionization of a weak acid HA is the ratio of the ionized acid concentration and initial concentration of the acid. Since the ionized acid concentration is the same as hydronium ion concentration, percent ionization is given by:

Let's designate the monoprotic weak acid as HA. HA dissociates in water to form H3O+ and A. From this, we can set up an ICE table for the equilibrium expression.

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The Ka of a monoprotic weak acid is 8.15 × 10-3. What is the percent ionization of a 0.146 M solution of this acid?

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