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 |
An analytical chemist is titrating 159.4mL of a 0.2300M solution of methylamine CH3NH2 with a 0.1600M...
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