Question

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=?

Answer #1

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.

Calculate the pH at the equivalence point for the titration of
.100M methylamine (CH3NH2) with .100 M HCL. The Kb of methylamine
is 5.0x10^-4

Calculate the pH at the equivalence point in the titration of
50.0 mL of 0.125 M methylamine (Kb = 4.4 × 10−4) with 0.265 M
HCl..

Calculate the pH at the equivalence point for the following
titration: 0.40 M HCl versus 0.40 M methylamine (CH3NH2). The Ka of
methylammonium is 2.3 × 10^−11

Calculate the pH at the equivalence point for the following
titration: 0.40 M HCl versus 0.40 M methylamine (CH3NH2). The Ka of
methylammonium is 2.3 × 10^−11

Calculate the pH at the equivalence point for the following
titration: 0.35 M HCl versus 0.35 M methylamine (CH3NH2). The Ka of
methylammonium is 2.3 × 10−11.

Consider the titration of a 26.0-mL sample of 0.180 M CH3NH2
with 0.145 M HBr. (The value of Kb for CH3NH2 is
4.4×10−4.)
Part A
Determine the initial pH.
Part B
Determine the volume of added acid required to reach the
equivalence point. answer to 3 sig figs
Part C
Determine the pH at 6.0 mL of added acid
Part D
Determine the pH at one-half of the equivalence point.
Part E
Determine the pH at the equivalence point.
Part...

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+]=

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