Question

Calculate the pH of a solution prepared by mixing equal volumes
of 0.17 M methylamine (CH3NH2, *K*b = 3.7×10−4) and 0.60 M
CH3NH3Cl.

Express your answer using two decimal places.

Answer #1

Calculate the pH of a solution that results from mixing 27 mL of
0.13 M methylamine (CH3NH2) with 27 mL of
0.11 M CH3NH3Cl. The Kb value for
CH3NH2 is 3.6 x 10-4.

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.

Part A
Find [OH−] of a 0.33 M methylamine (CH3NH2) solution.
(Methylamine has a Kb value of 4.4×10−4.)
Express the concentration in moles per liter to two significant
figures.
Part B
Find the pH of the 0.33 M methylamine (CH3NH2)
solution.
Express the pH of the solution to two decimal places

Calculate the pH of the following solutions. A solution is
prepared by mixing equal volumes of 0.15 M HCl and 0.53 M HNO3.
(Assume that volumes are additive.)

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 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.

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