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Home/ Questions/Calculate the percent dissociation of HA in a 0.10 M solution
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lizawr
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lizawr
Asked: April 10, 20222022-04-10T08:15:38+00:00 2022-04-10T08:15:38+00:00In: Chemistry

Calculate the percent dissociation of HA in a 0.10 M solution

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A certain weak acid, HA, has a Ka value of 9.9×10^-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


♦ Relevant knowledge
The term “weak acid” refers to a compound which ionizes in part in its constituent ions once it is dissolved in water. Examples of weak acids include Oxalic acid Phosphoric Acid and Nitrous Acid. Methanoic acid (Formic Acid), Ethanoic acid (Acetic acid), Ascorbic acid (Vitamin C) as well as Water.

Ka in chemistry refers to an indicator of how much an acid breaks up. It is an equilibrium constant that is called acid dissociation/ionization constant. This constant provides information on the strength of acid. The greater it is the Ka number, the more powerful the acid. It’s based on the notion of strong acids being more likely to completely dissociate, resulting in high dissociation values for Ka. Strong acids break up completely while weak acids only dissociate only a small amount.

dissociationka valueweak acid
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    tonytutoria
    2022-04-10T09:00:54+00:00Added an answer on April 10, 2022 at 9:00 am
    (1) Ans:
    Calculate the percent dissociation of HA in a 0.10 M solution
    (2) Ans:
    Calculate the percent dissociation of HA in a 0.10 M solution
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  2. tonytutoria
    2022-04-10T08:15:40+00:00Added an answer on April 10, 2022 at 8:15 am

    HA + H2O = H3O + A
    For a 0.10M solution:

    Where x is the concentration change:

    Ka = [H3O] [A]/[HA]

    9.9×10^-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 0.010M solution:

    Ka = [H3O] [A]/[HA]

    9.9×10^-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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  3. tonytutoria
    2022-04-10T08:15:41+00:00Added an answer on April 10, 2022 at 8:15 am

    We all know that weak acids will cause dissociation.

    Ha –>H+ + A-

    The Ka = [H+][A] / [HA]

    Initial conc. HA = 0.1

    let at equilbirium

    HA dissociated = x, so the conc will now be 0.1-x

    [H+] =[A-] =x

    So Ka = x 2 / 0.1-x

    We can ignore x in deonimator because the acid is weak.

    So

    7.0

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