Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.11. Also, find the percent dissociation of this solution.
Added by Philip K.
Step 1
Given that the concentration of the weak monoprotic acid is 0.150 M, we can assume that [H+] is equal to the concentration of the acid. Therefore, [H+] = 0.150 M. Now, calculate the pH using the formula: pH = -log(0.150) = -(-0.823) = 0.823 Show more…
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