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Determine [H3O+] and [OH-] concentrations (in M to two decimal places) for each: a) Pure water...

Determine [H3O+] and [OH-] concentrations (in M to two decimal places) for each: a) Pure water at 10 degrees C (Kw=0.293 x 10^-14) Answers:5.41 x 10^-8 M and 5.41 x 10^-8. b) An aqueous solution with a pH of 3.23 Answers: 5.89 x 10^-4 M and 1.70 x 10^-11 M Please show all work

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Answer #1

a)

Kw = [H3O+][OH-]

Since water is pure, it will be neutral and [H3O+] = [OH-]

So,

Kw = [H3O+][H3O+]

Kw = [H3O+]^2

0.293*10^-14 = [H3O+]^2

[H3O+] = 5.41*10^-8 M

So,[OH-] = 5.41*10^-8 M

5.41*10^-8 M

5.41*10^-8 M

b)

use:

pH = -log [H3O+]

3.23 = -log [H3O+]

[H3O+] = 5.89*10^-4 M

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)/(5.89*10^-4)

[OH-] = 1.70*10^-11 M

5.89*10^-4 M

1.70*10^-11 M

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