For each of the following strong base solutions, determine [OH?],[H3O+], p H , a
ID: 1033096 • Letter: F
Question
For each of the following strong base solutions, determine [OH?],[H3O+], pH, and pOH.
Part A
8.87×10?3 M LiOH
Part B
Express your answer to three decimal places. Enter your answers numerically separated by commas.
pH,pOH =
Part C
1.10×10?2 M Ba(OH)2
Express your answer using three significant figures. Enter your answers numerically separated by commas.
[OH?],[H3O+] =
Part D
Express your answer to three decimal places. Enter your answers numerically separated by commas.
pH,pOH =
Part E
2.0×10?4 M KOH
Express your answer using two significant figures. Enter your answers numerically separated by commas.
Part F
Express your answer to two decimal places. Enter your answers numerically separated by commas
Part G
5.3×10?4 M Ca(OH)2
Express your answer using two significant figures. Enter your answers numerically separated by commas.
[OH?],[H3O+] =
Part H
Express your answer to two decimal places. Enter your answers numerically separated by commas.
[OH?],[H3O+] =Explanation / Answer
A)
[OH-] = [LiOH] = 8.87*10^-3 M
use:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
= (1.0*10^-14)/(8.87*10^-3)
= 1.13*10^-12 M
Answer:
[OH-] = [LiOH] = 8.87*10^-3 M
[H3O+] = 1.13*10^-12 M
B)
use:
pH = -log [H3O+]
= -log (1.13*10^-12)
= 11.948
use:
pOH = -log [OH-]
= -log (8.87*10^-3)
= 2.052
Answer:
pH = 11.948
pOH = 2.052
C)
[OH-] = 2*(Ba(OH)2) = 2*1.10*10^-2 = 2.20*10^-2 M
use:
[H3O+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H3O+] = (1.0*10^-14)/[OH-]
= (1.0*10^-14)/(2.20*10^-2)
= 4.54*10^-13 M
Answer:
[OH-] = 2.20*10^-2 M
[H3O+] = 4.54*10^-13 M
D)
use:
pH = -log [H3O+]
= -log (4.545*10^-13)
= 12.342
use:
pOH = -log [OH-]
= -log (2.2*10^-2)
= 1.658
Answers:
pH = 12.342
pOH = 1.658
only 4 parts at a time
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