Question

the pH of .10 M ethylamine is 11.82

a) Calculate the Kb for ethyamine using the information provided

b) based on your answer in (a) calculate the pH of .15 ethylammonium chloride

Answer #1

Calculate the pH of a 0.0416 M aqueous solution of ethylamine
(C2H5NH2, Kb = 4.3×10-4) and the equilibrium concentrations of the
weak base and its conjugate acid.
pH
=
[C2H5NH2]equilibrium
=
M
[C2H5NH3+
]equilibrium
=

#2 Ethylamine (CH3CH2NH2) is a
base compound.
a) Write base dissociation reaction ethylamine.
b) If Kb of ethylamine is 7.41x10-10 ,
what is the pH of 0.15 M ethylamine solution?

Find the [OH−] in a 0.340 M solution of ethylamine (C2H5NH2).
For ethylamine, Kb=5.6⋅10−4.

Calculate the molar concentration of OH- ions in a
8.1 x 10-2 M solution of ethylamine (Kb= 6.4
x 10-4).
Calculate the pH of this solution.

Calculate the expected pH of a 0.100 M solution of ammonium
chloride given that Kb for ammonia is
1.76x10-5

Calculate the pH of a 0.22 M CH3NH3Br solution. Kb(CH3NH2) = 4.4
×10–4

Calculate the pH of a 0.0786 M aqueous solution of the weak base
caffeine (C8H10N4O2, Kb = 4.10×10-4). pH Calculate the pH of a
0.0786 M aqueous solution of the weak base
caffeine
(C8H10N4O2,
Kb = 4.10×10-4).
pH =

The pH of a 9.94×10-4 M solution of a weak base is 8.54.
Calculate Kb for this base to three significant figures.

Calculate the pH of a 0.166 M aqueous solution of pyridine
(C5H5N, Kb = 1.5×10-9) and the equilibrium concentrations of the
weak base and its conjugate acid.
pH =
[C5H5N]equilibrium = M
[C5H5NH+]equilibrium = M

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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