Calculate the pH of a 0.75 M acetic acid solution, CH3COOH, Ka = 1.8 x 10–5, and compare it with the calcul?
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Calculate the pH of a 0.75 M acetic acid solution, CH3COOH, Ka = 1.8 x 10^–5, and compare it with the calculated pH of a 0.75 M diethylamine solution, (CH3CH2)2NH, Kb = 7.1 x 10^–4. What is the ratio of the hydronium ion concentrations in each solution?
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the pH of a 0.75 M acetic acid solution
[H+] = sqrt(Ka M) = sqrt(1,8 10^-5 x 0.75) = 3.7 10^-3
pH = -log_10 3.7 10^-3 = 2.43
pH of a 0.75 M diethylamine solution
[OH-] = sqrt: Kbx M) = sqrt (7.1 10^-4 x 0.75) = 2.3 10^-2
pOH = -log_10 2.3 10^-2 = 1.64
pH = 14 - 1.64 = 12.36
the ratio of the hydronium ion concentrations in each solution = 10^-2.43 / 10^-12.36 = 8.5 x 10^9
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