Question

Calculate the pH and concentrations of CH3NH2 and CH3NH3 in a 0.0275 M methylamine (CH3NH2) solution. The Kb of CH3NH2 = 4.47 × 10-4.

Answer #1

Calculate the pH and concentrations of CH3NH2 and CH3NH3 in a
0.0367 M methylamine (CH3NH2) solution. The Kb of CH3NH2 = 4.47 ×
10-4.
pH=
[CH3NH2]=
[CH3NH3+]=

A 0.108-M aqueous solution of CH3NH2 (methylamine) has a pH of
11.8. Calculate the pH of a buffer solution that is 0.108 M in
CH3NH2 and 0.308 M in CH3NH3+

Calculate OH- and pH in a solution in which CH3NH2 is 0.300 M
and CH3NH3+ is: (kb ch3nh2: 4.2 x 10^-4
A). 0.0500 M
B). 0.200 M
C). 0.300 M
D).0.500 M
Please show steps.

Determine the PH of a 2.75 M aqueous solution of
CH3NH2 (methylamine). The Kb of methylamine
is 4.4x10-4.

Calculate the pH at the equivalence point for the titration of
0.180 M methylamine (CH3NH2) with 0.180 M HCl. The Kb of
methylamine is 5.0× 10–4.
pH=?

Calculate the pH of a solution prepared by mixing equal volumes
of 0.17 M methylamine (CH3NH2, Kb = 3.7×10−4) and 0.60 M
CH3NH3Cl.
Express your answer using two decimal places.

Calculate the pH of a 0.50 M solution of
methylamine(CH3NH2, Kb = 4.4 x
10-4.)
a.
1.83
b.
10.64
c.
12.17
d.
5.47
e.
8.53

Calculate the pH at the equivalence point for the titration of
0.130 M methylamine (CH3NH2) with 0.130 M HCl. The Kb of
methylamine is 5.0× 10–4.

Calculate the pH at the equivalence point for the titration of
0.240 M methylamine (CH3NH2) with 0.240 M HCl. The Kb of
methylamine is 5.0× 10–4.

Calculate the pH at the equivalence point for the titration of
0.110 M methylamine (CH3NH2) with 0.110 M HCl. The Kb of
methylamine is 5.0× 10–4.

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