You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH_3COOH)

Question

You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH_3COOH) and 0.20 M sodium acetate (CH_3COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a = 1.8 10^-5] 4.65 4.71 4.56 4.84 5.07 Calculate the percent ionization of cyanic acid, K_a = 2.0 10^-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO. 0.02% 0.10% 0.20% 2.0% 20% In which one of the following solutions will acetic acid have the greatest ionization? 0.1 MCH_3COOH

Explanation / Answer

pKa = -log (2 x 10^-4)

        = 3.70

pH = pKa + log [salt / acid]

     = 3.70 + log (0.1 / 0.5)

     = 3.00

pH = -log[H+]

[H+] = 10^-pH = 10^-3

[H+] = 1 x 10^-3 M

percent ionization % = ( [H+] / initial) x 100

                                 = (1 x 10^-3 / 0.5) x 100

                                  = 0.2 %

answer : c) 0.2 %

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