Answer to Question #176468 in Physical Chemistry for A Hinds

Question

.      A 20.00 ml portion of o 0.1000 M butanoic acid (CH₃CH₂CH₂CO₂H), [K_a = 1.54 x 10^-5] was titrated with 0.1000 M NaOH solution.

(a)    Determine the pH of the solution after the addition of 15 ml of NaOH

(b)    What would be a likely pH of the solution at equivalence? Explain your answer.                                                                                         

(c)     Name a suitable indicator for this titration. Justify your answer.

Answer 1

a) pH of the solution =$4.82M$

b) $pH-pOH=14-4.82=9.18M$

When all of a weak acid has been neutralized by strong base, the solution is essentially equivalent to a solution of the conjugate base of the weak acid.

c) The pH quickly changes from 3 to 11.