n the laboratory, a general chemistry student measured the pH of a 0.342 M aqueous solution of ethylamine, C2H5NH2 to be 12.067.
Use the information she obtained to determine the Kb for this base.
1 answer:
Answer:
The value of
of the an ethylamine is
.
Explanation:
The pH of the solution = 12.067
The pOH of the solution = 14 - pH =14-12.607 =1.933
![pOH=-\log[OH^-]](https://tex.z-dn.net/?f=pOH%3D-%5Clog%5BOH%5E-%5D)
![1.933=-\log[OH^-]](https://tex.z-dn.net/?f=1.933%3D-%5Clog%5BOH%5E-%5D)
![[OH^-]=0.0117 M](https://tex.z-dn.net/?f=%5BOH%5E-%5D%3D0.0117%20M)

Initially
0.342 M 0 0
At equilibrium
(0.342-x) x x
The value of x = ![[OH^-]=0.0117 M](https://tex.z-dn.net/?f=%5BOH%5E-%5D%3D0.0117%20M)
The expression of
is given as:
![K_b=\frac{[C_2H_5NH_3^{+}][OH^-]}{[C_2H_5NH_2]}](https://tex.z-dn.net/?f=K_b%3D%5Cfrac%7B%5BC_2H_5NH_3%5E%7B%2B%7D%5D%5BOH%5E-%5D%7D%7B%5BC_2H_5NH_2%5D%7D)


The value of
of the an ethylamine is
.
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