Calculate the ph of an aqueous solution at 25°c that is 0.31 m in phenol (c6h5oh). (ka for phenol = 1.3 × 10−10.)

Given:

Concentration of phenol = 0.31 M

Ka (acid dissociation constant) = 1.3 * 10⁻¹⁰

To determine:

The pH of the solution

Explanation:

            C6H5OH ↔ C6H5O⁻ + H⁺

Initial       0.31 M          0             0

change   -x                 +x             +x

Equlib        0.31-x         x             x

Ka = [C6H5O⁻][H⁺]/[C5H5OH]

1.31*10⁻¹⁰ = x²/0.31-x

x =[H+]= 6.37*10⁻⁶M

pH = -log[H+] = -log(6.37*10⁻⁶) = 5.19

Ans: pH of the solution is 5.19

pH of the solution is 5.19

answer; i believe that the correct answer is (a) potassium(k)

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.