Problem: What is the pH of a 0.200 M aqueous solution of phenol, H5C6OH, (Ka = 1.0 x 10-10)?A. 0.70B. 5.3C. 7.0D. 10.E. none of the above

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We are being asked to calculate the pH of a 0.200 M aqueous solution of phenol, H5C6OH, (Ka = 1.0 x 10-10).

H5C6OH weak acidproton donor
H2O → will act as the weak baseproton acceptor

Equilibrium reaction:        H5C6OH(aq) + H2O(l)  H5C6O-(aq) + H3O+(aq)


We're going to calculate for the pH of the solution using the following steps:

Step 1: Construct an ICE chart for the reaction.
Step 2: Write the Ka expression and calculate for Ka.
Step 3: Calculate the H3O+ concentration.
Step 4: Calculate for pH.

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Problem Details

What is the pH of a 0.200 M aqueous solution of phenol, H5C6OH, (Ka = 1.0 x 10-10)?

A. 0.70

B. 5.3

C. 7.0

D. 10.

E. none of the above

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