The pOH of an aqueous solution at 25°C was found to be 8.80 . The pH of this sol
ID: 998856 • Letter: T
Question
The pOH of an aqueous solution at 25°C was found to be8.80.
The pH of this solution is .
The hydronium ion concentration is M.
The hydroxide ion concentration is M.
The pH of an aqueous solution at 25°C was found to be 8.50.
The pOH of this solution is .
The hydronium ion concentration is M.
The hydroxide ion concentration is M.
What is the pOH of an aqueous solution of 0.323 M perchloric acid?
pOH = M
What is the hydronium ion concentration in an aqueoushydroiodic acid solution with a pH of 1.680?
[H3O+] = M
What is the hydronium ion concentration in an aqueousperchloric acid solution that has a pOH of 9.700?
[H3O+] = M
Explanation / Answer
Answer – 1) We are given, pOH = 8.80
We know,
pH +pOH = 14
so, pH = 14 – pOH
= 14 – 8.80
= 5.20
Now hydronium ion
We know,
pH = -log [H3O+]
[H3O+] = 10-pH
= 10-5.2
= 6.31*10-6 M
Hydroxide ion –
We know,
pOH = -log [OH-]
[OH-] = 10-pOH
= 10 -8.80
= 1.58*10-9 M
2) We are given, pH = 8.50
We know,
pH +pOH = 14
so, pOH = 14 – pH
= 14 – 8.50
= 5.50
Now hydronium ion
We know,
pH = -log [H3O+]
[H3O+] = 10-pH
= 10-8.50
= 3.16*10-9 M
Hydroxide ion –
We know,
pOH = -log [OH-]
[OH-] = 10-pOH
= 10 -5.50
= 3.16*10-6 M
3) We are given the [HClO4] = 0.324 M
We know perchloric acid strong acid, so [HClO4] = [H3O+]
So, [H3O+] = 0.324 M
We know,
pH = -log [H3O+]
= -log 0.324 M
= 0.489
We know,
pH +pOH = 14
so, pOH = 14 – pH
= 14 – 0.489
= 13.5
4) We are given, pH = 1.680
We know,
pH = -log [H3O+]
[H3O+] = 10-pH
= 10-1.680
= 0.0209 M
5) We are given, pOH = 9.700
We know,
pH +pOH = 14
so, pH = 14 – pOH
= 14 – 9.70
= 4.3
Now hydronium ion
We know,
pH = -log [H3O+]
[H3O+] = 10-pH
= 10-4.3
= 5.01*10-5 M
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