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Law Incorporation [45]
3 years ago
14

Using the average initial pH of your acetic acid solutions (2.96), and the average molarity of those solutions(.0602), calculate

a value of Ka for acetic acid. Report your result to 3 significant figures.
Chemistry
1 answer:
Orlov [11]3 years ago
3 0

Answer : The value of Ka for acetic acid is,  2.03\times 10^{-5}

Explanation :

The chemical formula of acetic acid is, CH_3COOH.

The chemical equilibrium reaction will be:

CH_3COOH\rightleftharpoons CH_3COO^-+H^+

Given:

pH = 2.96

First we have to calculate the concentration of hydrogen ion.

pH=-\log [H^+]

2.96=-\log [H^+]

[H^+]=1.096\times 10^{-3}M

That means,

[H^+]=[CH_3COO^-]=1.096\times 10^{-3}M

[CH_3COOH]=0.0602-(1.096\times 10^{-3})=0.0591M

The expression for reaction is:

K_a=\frac{[CH_3COO^-][H^+]}{[CH_3COOH]}

K_a=\frac{(1.096\times 10^{-3})\times (1.096\times 10^{-3})}{0.0591}

K_a=2.03\times 10^{-5}

Thus, the value of Ka for acetic acid is,  2.03\times 10^{-5}

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