If the Ka of a monoprotic weak acid is 6.8 × 10−6, what is the pH of a 0.11 M solution of this acid?
pH of the solution of a weak acid = 1/2 pKa - 1/2 log C where pKa = - log Ka and C = concentration.
Given, Ka = 6.8 x 10-6 and C = 0.11 M
So, pKa = 5.167
and pH = (5.167/2) - (log(0.11)/2)
= 2.58 - (-0.47) = 3.05
If the Ka of a monoprotic weak acid is 6.8 × 10−6, what is the pH...
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