Question

what is the ph of 0.1M of acetic acid

Answer 1

Hy.......


As Acetic Acid is a weak acid, it doesn’t completely dissociate in an aquous solution. It dissociates partially. And the amount of dissociated H+ ions can be counted using Ostwald’s Dilution Law.

The Ka value for acetic acid, CH3COOH(aq), is 1.8x10^-5

so, using Ostwald’s Dilution Law and pH Scale Definition,

we can write=> pH=−log(sqrt(Ka∗C))pH=−log(sqrt(Ka∗C))

where, C=0.1 M

so, pH=2.87 (by calculating)



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Answer 2

In solution, it has a pKa value of 4.76. Its conjugate base is acetate (CH3COO−). A 1.0 M solution has a pH of 2.4, indicating that merely 0.4% of theacetic acid molecules are dissociated. The required pH of 0.1 M solution of acetic acid is 2.88.
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