Question

An analytical chemist is titrating

159.4mL

of a

0.2300M

solution of methylamine

CH3NH2

with a

0.1600M

solution of

HNO3

. The

pKb

of methylamine is

3.36

. Calculate the pH of the base solution after the chemist has added

91.4mL

of the

HNO3

solution to it.

Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of

HNO3

solution added.

Round your answer to

2

decimal places.

=pH

Answer 1

If any queries regarding this solution please comment here.

Answer 2