Question

Give the hydronium ion and hydroxide ion concentrations of solutions with the following values of pH.

1. pH 13.0 for (H3O+)

2. pH 13.0 for OH-

3. pH 3.0 for H3O+

4. pH 3.0 for OH-

5. pH 10.0 for H3O+

6. pH 10.0 for OH-

Answer 1

1)

we have below equation to be used:

pH = -log [H3O+]

13 = -log [H3O+]

log [H3O+] = -13

[H3O+] = 10^(-13)

[H3O+] = 1.000*10^-13 M

Answer: 1.000*10^-13 M

2)

we have below equation to be used:

[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)/(1*10^-13)

[OH-] = 0.1000 M

Answer: 0.1000 M

3)

we have below equation to be used:

pH = -log [H3O+]

3 = -log [H3O+]

log [H3O+] = -3

[H3O+] = 10^(-3)

[H3O+] = 1.00*10^-3 M

Answer: 1.00*10^-3 M

4)

[OH-] = (1.0*10^-14)/[H3O+]

[OH-] = (1.0*10^-14)/(1*10^-3)

[OH-] = 1.00*10^-11 M

Answer: 1.00*10^-11 M

5)

we have below equation to be used:

pH = -log [H3O+]

10 = -log [H3O+]

log [H3O+] = -10

[H3O+] = 10^(-10)

[H3O+] = 1.000*10^-10 M

Answer: 1.000*10^-10 M

6)

[OH-] = (1.0*10^-14)/[H3O+]

[OH-] = (1.0*10^-14)/(1.000*10^-10)

[OH-] = 1.000*10^-4 M

Answer: 1.000*10^-4 M