If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the pH of a 0.46 M solution of this acid?
For weak monoprotic acids [H+] = sqrt( Ka X C)
[H+] = sqrt( 4.7 X 10-6 X 0.46)
[H+] = 1.47 X 10-3 M
pH = -log[H+]
= -log [1.47 X 10-3]
pH = 2.8327
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