Calculate the percent ionization of a 0.381 M solution of hydrocyanic acid.

Question

Calculate the percent ionization of a 0.381 M solution of hydrocyanic acid.

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RuslanHeatt 4 years 2021-08-26T20:47:49+00:00 1 Answers 14 views 0

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  1. Orla
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    2021-08-26T20:49:07+00:00
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    Answer:

    .00402 %

    Explanation:

    hydrocyanic acid (HCN) is a weak acid with a Ka of 6.17*10^-10 so you need to do a RICE table

    initial concentration of HCN is .381 and initial H+ and CN- concentration is 0.

    that means the equillibrium concentration of HCN will be (.381-x) and H+ and CN- will be x

    put that into the formula for Ka, so it’ll be Ka = x^2/(.381-x) and then use quadratic equation to solve. You’ll end up getting x = 1.5 * 10^-5.

    Then to find percent ionization you solve (concentration of formed ions / initial HCN)

    Which will be (1.5 * 10^-5 / .381) * 100 = .00402 % making it a very weak acid <3

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