Question

A 0.200 M solution of a weak acid, HA, is 9.4% ionized. Using this information, calculate Ka for HA.

Answer #1

**Answer** – We are given, percent ionization = 9.4
% , [HA] = 0.200 M

We know formula for percent ionization,

Percent ionization = x/ initial concentration of HA *100 %

x = ionized species concentration =
[H_{3}O^{+}]

So,

10 % = x / 0.200 * 100 %

x = 9.4 %*0.200 / 100 %

= 0.0188 M

X = [H_{3}O^{+}] = [HA^{-}] = 0.0188
M

So, **[HA]** = 0.200 - 0.0188 M

= **0.181 M**

We know,

**Ka**
=[H_{3}O^{+}][HA^{-}] / [HA]

= 0.0188 *0.0188 / 0.181

=
**1.95*10 ^{-3}**

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Calculate (a) the Ka, (b) the pH of the solution, and (c) the
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B) Calculate the percent ionization of HA in a 0.010 M
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certain weak acid, HA, has a Ka value of
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Step-by-step mathematics when breaking apart the Ka equation
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Part A Calculate the percent ionization of HA
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