What is the fraction of HA dissociated at a pH of 6.10 if Ka = 1.8...

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What is the fraction of HA dissociated at a pH of 6.10 if Ka =1.8 x 10-5? 0% 4% 100% 96%
Which of the following is true about the shape of the titrationcurve for a 0.1 M weak acid being titrated with a 0.2 M strong baseas compared to a 0.1 M strong acid being titrated with a 0.2 Mstrong base?
The equivalence point volume will shift to the left.
It will start at a lower pH.
The equivalence point pH will be larger.
The equivalence point volume will shift to the right.
What is the volume at the equivalence point when 30.0 mL of 0.25M HCl are titrated with 0.40 M NaOH at T = 298 K? K_w =1.00 x 10^-14.
18.8 mL
30.0 mL
7.00 mL
37.6 mL

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3.8 Ratings (719 Votes)

pH = 6.10

[H+] = 10^-pH

Â Â Â Â Â Â Â = 10^-6.10

Â Â Â Â Â Â Â = 7.94 x 10^-7 M

Ka = [H+]^2 / C

1.8 x 10^-5 = (7.94 x 10^-7)^2 / C

C = 3.50 x 10^-8 M

fraction of HA dissociated = H+ x 100 / C

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 7.94 x 10^-7 x 100 / 3.50 x 10^-8

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 100%

answer : 100%

answer : The equivalence point pH will be larger

volume = 30 x 0.25 / 0.40 = 18.75 mL

answer : 18.8 mL

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What is the fraction of HA dissociated at a pH of 6.10 if Ka = 1.8...

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