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 acid → proton donor
• H2O → will act as the weak base → proton 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.
What is the pH of a 0.200 M aqueous solution of phenol, H5C6OH, (Ka = 1.0 x 10-10)?
E. none of the above