if the concentration of acetic acid is 0.10 m, what is the ph of the resulting solution?
a)-2.89
b)0.10
c)7.00
d)2.89

Option D) 2.89.

Explanation:

Look up the acid dissociation constant of acetic acid:

(CRC Handbook of Chemistry and Physics, 84th Edition (2004).)

Acetic acid partially dissociate to produce acetate ions and hydrogen ions:

.

Let the final concentration of in the solution be . The concentration of acetic acid would have dropped by and the concentration of acetate ions would have increased by . The initial concentration of in pure water is and will barely influence the outcome.

Construct a RICE table for this reaction: (all values here are in , which stands for concentrations in moles per liter.)

.

At equilibrium:

By the definition of the acid dissociation constant, :

.

That is:

.

Rearrange and solve for :

.

.

There might be more than one solution to this equation. However, keep in mind that all concentration should be positive (at least non-negative.) The only possible value of will thus be approximately .

In other words, at equilibrium . By the definition of pH,

.

Note that depending on the value, the final result might slightly vary.

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