Equivalence Point pH Calculation in Acid-Base Titration
What is the pH at the equivalence point of a 0.01M solution of strong acid titrated using 45mL of 0.02M of a strong base?
Answer:
Explanation:45 mL = .045 L .045 L of .02M base will contain .045 x .02 mole of base = .0009 mole of base acid = .01 mole net acid = .01 - .0009 = .0091 mole this mole has volume of .045L concentration of acidic solution = .0091 / .045 = .2022 M = 2022 x 10⁻⁴ M pH = - log 2022 x 10⁻⁴= 4 - log 2022= 4 - 3.3 = .7 pH = .7
Explanation: At the equivalence point of the titration between a strong acid and a strong base, the moles of the acid will be equal to the moles of the base. In this case, when 45mL of 0.02M strong base is titrated with 0.01M strong acid, the pH at the equivalence point is calculated to be 0.7.