Question

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.

Answer #1

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 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
.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.

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+]=

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.

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