Question

Calculate the pH of a 0.67 M methylamine solution.

Answer #1

Calculate the pH of a 0.21 M methylamine solution.

22. Calculate the pH of a 0.65 M methylamine solution. pH =
B. The pH of an acid solution is 5.46. Calculate the Ka for the
monoprotic acid. The initial acid concentration is 0.010 M. Ka = ×
10 Enter your answer in scientific notation.

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 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.

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

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.

Find the [OH-] and pH of a 0.66 M methylamine solution

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

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