If the [H+] in a solution is 1x10^-1 mol/L what is the [OH^-] ??
(H^+)(OH^-) = 1E-14.
Substitute H^+ and solve for OH^-
To determine the concentration of hydroxide ions ([OH-]) in a solution based on the concentration of hydronium ions ([H+]), you can use the equation for the ion product of water (Kw). The equation for the ion product of water is:
Kw = [H+][OH-]
At 25°C, the value of Kw is 1.0 x 10^-14 mol2/L2. Since we know the concentration of the hydronium ions ([H+]) in the solution is 1 x 10^-1 mol/L, we can rearrange the equation to solve for [OH-].
First, divide both sides of the equation by [H+]:
Kw / [H+] = [OH-]
Now, substitute the values:
(1.0 x 10^-14 mol2/L2) / (1.0 x 10^-1 mol/L) = [OH-]
Simplifying the equation, we get:
1.0 x 10^-13 mol/L = [OH-]
Therefore, the concentration of hydroxide ions ([OH-]) in the solution is 1.0 x 10^-13 mol/L.