![Calculate either [H,0+] or [OH-] for each of the solutions at 25 °C. Solution A: (OH) = 2.15 x 10-7M Solution A: 1,0+) = Solu](https://i.imgur.com/DDfN7lH.png)
Answers
A)
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-]
[H3O+] = (1.0*10^-14)/2.15*10^-7
[H3O+] = 4.651*10^-8 M
Answer: 4.65*10^-8 M
B)
use:
[OH-] = Kw/[H3O+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H3O+]
[OH-] = (1.0*10^-14)/(8.89*10^-9)
[OH-] = 1.125*10^-6 M
Answer: 1.12*10^-6 M
C)
use:
[OH-] = Kw/[H3O+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H3O+]
[OH-] = (1.0*10^-14)/(7.47*10^-4)
[OH-] = 1.339*10^-11 M
Answer: 1.34*10^-11 M
D)
For basic solution, [OH-] is greater than [H3O+]
This is true for A and B
Answer: Solution B, Solution A
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