Question

#2 Ethylamine (CH_{3}CH_{2}NH_{2}) is a
base compound.

a) Write base dissociation reaction ethylamine.

b) If K_{b} of ethylamine is 7.41x10^{-10} ,
what is the pH of 0.15 M ethylamine solution?

Answer #1

a)

CH3CH2NH2 +H2O -----> CH3CH2NH3+ + OH-

b)

Lets write the dissociation equation of CH3CH2NH2

CH3CH2NH2 +H2O -----> CH3CH2NH3+ + OH-

0.15 0 0

0.15-x x x

Kb = [CH3CH2NH3+][OH-]/[CH3CH2NH2]

Kb = x*x/(c-x)

Assuming small x approximation, that is lets assume that x can be ignored as compared to c

So, above expression becomes

Kb = x*x/(c)

so, x = sqrt (Kb*c)

x = sqrt ((7.41*10^-10)*0.15) = 1.054*10^-5

since c is much greater than x, our assumption is correct

so, x = 1.054*10^-5 M

So, [OH-] = x = 1.054*10^-5 M

we have below equation to be used:

pOH = -log [OH-]

= -log (1.054*10^-5)

= 4.98

we have below equation to be used:

PH = 14 - pOH

= 14 - 4.98

= 9.02

Answer: 9.02

The drug codeine is an alkaloid - a basic organic compound. The
Kb for codeine is 1.62 x 10-6
a.) Write the reaction equation for the reaction of codeine with
water, using "R3N" for codeine.
Reaction:
_________________________________________________________
b.) Is codeine a weak base or a strong base? What does this mean
for the reaction in 5a?
_____________________________________________________________________.
c.) What are the pH and pOH of a 3.42 x 10-4 M
solution of codeine?
pH=_________ pOH=_____________ Is this
solution acidic, basic...

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
=

Part 1:
a) write the ka reaction for HCNO.
b) write the equilibrium constant expression for the
dissociation of HCNO.
c) Construct (don't solve) the ICE chart for the acid
dissociation of 0.100 M HCNO.
d) what is the pH of a 0.100 M HCNO solution.
Part II:
a) Write the base dissociation reaction of HONH2.
b) write the equilibrium constant expression for the base
dissociation of HONH2.
c) Construct (don't solve) the ICE chart for the acid
dissociation of...

A 0.0884 M solution of a weak base has a pH of 11.79. What is
the identity of the weak base? Weak Base Kb Ethylamine (CH3CH2NH2)
4.7 X 10–4 Hydrazine (N2H4) 1.7 X 10–6 Hydroxylamine (NH2OH) 1.1 X
10–8 Pyridine (C5H5N) 1.4 X 10–9 Aniline (C6H5NH2) 4.2 X 10–10

1)The compound dimethylamine is a weak base
like ammonia. A solution contains 0.205 M
(CH3)2NH2+
and 0.295 M
dimethylamine,
(CH3)2NH.
The pH of this solution is .
2)The compound ethylamine is a weak base like
ammonia. A solution contains 0.461 M
C2H5NH3+
and 0.367 M ethylamine,
C2H5NH2.
The pH of this solution is .

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

Dimethylamine ((CH3 )2NH) is a weak base
with Kb = 5.1 × 10−4. What
is the pH of a 0.60 M solution of dimethylamine
and what is the percent dissociation?

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

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 pH of a weak base solution ([B]0 >
100 • Kb
Calculate the pH of a 0.106 M aqueous solution of
triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium
concentrations of the weak base and its conjugate acid.

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