Concentration and pH?

Question

What is the hydroxide ion concentration in an aqueous solution if the hydronium ion concentration is 1 x 10^-5 mole per liter? What is the pH of the solution?

Any help would be greatly appreciated

Answer 1

The pH of an aqueous solution is equal to - log [H3O+]

pH = - log [1x10^-5] = 5

In an aqueous solution, the concentration of the hydroxide ion multiplied by the concentration of the hydronium ion is equal to 1x10^-14.

In equation form;

[OH-]*[H3O+] = 1x10^-14

Rearrange to solve for [OH-] to get

[OH-] = 1x10^-14 / [H3O+]
[OH-] = 1x10^-14 / [1x10^-5]

[OH-] = 1x10^-9 mol / L

Answer 2

To find the OH- concentration simply take the H+ concentration and subtract that from 1 x 10^-14, so in this case the OH- concentration would be 1 x 10^-9.

to find the pH on a substance you need to take the -log[H+]
so it would be -log [1 x 10^-5] which gives you 5

Answer 3

in water hydronium (H3O+) and hydroxide (OH-) ions are in equilibrium according to

Kw = [H3O+][OH-] = 10^-14

given [H3O+] = 10^-5, [OH-] = 10^-14 / 10^-5 = 10^-9 mol/L

the pH is given by

pH = -log10([H3O+]) = 5

Answer 4

Kw = [H+][OH-] = 10^-14 M
so [OH-] = 10^-14 / 1x10^-5 = 10^-9 mole per liter
pH = - log [H+] = - log (1x10^-5) = 5

Answer 5

For the 1st question, it ability the acid provides better than one H+ ion in step with acid molecule. For the 2nd question, the acid in straight forward terms slightly dissociates into the H+ and anion compound