Final answer:
The concentration of [H3O+] for a 0.153 M solution of benzoic acid is known to be 0.00245 M. The pH of this solution is calculated to be 2.61.
Step-by-step explanation:
Acid-base equilibrium is the state of balance between the forward and reverse reactions of acids and bases in solution12. The strength of acids and bases depends on their tendencies to donate or accept protons. The extent of the acid-base reaction can be measured by an equilibrium constant K c, which reflects the relative concentrations of the products and reactants at equilibrium.
The concentration of [H3O+] in a solution of benzoic acid can be determined by applying the square root of the product of the reaction constant (Ka) and the concentration of the solution. In this case, [H3O+] = √((6.5×10−5) × 0.153 M) = 0.00245 M. Then, we calculate the pH by taking the negative log of the [H3O+]. So, pH = -log(0.00245) = 2.61(after rounding to two decimal places).
Learn more about Acid-Base Equilibrium