Question

What are the concentrations of OH and H+ in a 0.00072 M solution of Ba(OH), at 25 °C? Assume complete dissociation. [OH-] = [H+] = {

Answer 1

1 Ba(OH)2 has2 OH-

So,

[OH-] = 2*[Ba(OH)2]

= 2*0.00072 M

= 1.44*10^-3 M

use:

[H+] = Kw/[OH-]

Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC

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

[H+] = (1.0*10^-14)/1.44*10^-3

[H+] = 6.944*10^-12 M

Answer:

[OH-] = 1.4*10^-3 M

[H+] = 6.9*10^-12 M