What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x 10^-10)?

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Chemistry

What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x10^-10)?

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C6H5OHÂ Â Â ----------------------------> C6H5O- + H+

0.11Â 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 Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0 ----------------> initial

0.11-xÂ 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 Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â x -------------------> equilibrium

Ka = [C6H5O-][H+]/[C6H5OH]

Ka = x^2 / 0.11-x

1.3 x 10^-10 = x^2 / 0.11-x

x^2 + 1.3 x 10^-10 x -1.43 x 10^-11 = 0

by solving this

x = 3.78 x 10^-6

[H+] = x = 3.78 x 10^-6 M

pH = -log [H+] = -log (3.78 x 10^-6)

pH = 5.42 -----------------------> answer

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What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x 10^-10)?

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80.2K

Verified Solution

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Chemistry

What is the pH of a 0.11 M solution of C6H5OH (Ka = 1.3 x10^-10)?

Answer & Explanation Solved by verified expert

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