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12 Dec 2019

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The percent ionization of a solution is determined by: percent ionization =concentration of ionized acid/initial concentration of acid×100% Determined the percent ionization of a 0.098 M HF solution. The Ka value for HF is 3.5×10−4.

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Related questions

Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid.

Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.)

Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.)

Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.)

Part E Find the [H3O+] concentration of a 0.281 M acetic acid solution. (The value of Ka for acetic acid is 1.8×10−5.)

Find the percent ionization of a 0.337 M HF solution. The Ka for HF is 3.5 × 10-4. What would you expect the percent ionization to be for the same concentration of hydrochloric acid (HCl)? Explain.

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