Solution Found!
Calculate [H3O+] for each solution.(a) pH = 8.55(b) pH = 11.23(c) pH = 2.87(d) pH = 1.22
Chapter 14, Problem 71P(choose chapter or problem)
Calculate \(\mathrm{[H_3O^+]}\) for each solution.
(a) pH = 8.55
(b) pH = 11.23
(c) pH = 2.87
(d) pH = 1.22
Questions & Answers
QUESTION:
Calculate \(\mathrm{[H_3O^+]}\) for each solution.
(a) pH = 8.55
(b) pH = 11.23
(c) pH = 2.87
(d) pH = 1.22
ANSWER:Solution:
The concentration of [OH-] ion and [H3O+] can be determined as follows ,
It is known that pH = -log [H3O+]
-pH = log [H3O+]
10 -pH = 10log [H3O+] or
[H3O+] = 10-pH
1.0 10-14
And [OH- ] = --------------
[H3O+]
Step 1
(a) pH = 8.25
pH = 8.25
The [H3O+] from pH = 8.25 can be calculated as follows,
[H3O+] = 10-pH or [H3O+] = antilog (- pH)
8.25 = - log [H3O+]
- 8.25 = log [H3O+]
[H3O+] = 10- 8.25 = 5.62 10-9 M
1.0 10-14 1.0 10-14
Thus, [OH-] = -------------- = ----------- = 1.710-6M
[H3O+] 5.62 10-9
(b) pH = 11.23