Question

A 50.0 50.0 mL solution of 0.127 0.127 M KOH KOH is titrated with 0.254 0.254 M HCl HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCl HCl.

Answer 1

Answer:

Explanation:

THE CORECT QUESTION

A 50.0 mL solution of 0.127 M KOH is titrated with 0.254 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCl.

SOLUTION

Get the concentration of the HCl first using titration formula

CA X V A / CB VB = NA/ NB

Equation of reation; KOH + HCl => KCl + H2O

CA = 0.254 M

CB = 0.127

VA = 1/0.254 = 3.937

CA (after the addition) = 0.127 x 50 / 3.937

                                     = 1.612 M

But pH = - Log[hydrogen ion]

            = -log 1.612

            =