What are [H+] and [OH-] for 0.01 M perchloric acid?
HClO4 is a strong acid; it ionizes 100%. Therefore, (H^+) = (HClO4)
(H^+)(OH^-) = 1E=14
I don't quite under stand that answer..
To find the concentrations of hydrogen ions ([H+]) and hydroxide ions ([OH-]) for a given acid, you need to use the concept of dissociation. In the case of perchloric acid (HClO4), it is a strong acid that completely dissociates in water. Because of this, the concentration of [H+] equals the initial concentration of the acid, while the concentration of [OH-] is determined by the autoionization of water.
The autoionization of water involves the reaction:
H2O ⇌ H+ + OH-
In pure water, the concentration of [H+] and [OH-] are equal due to the law of constant proportions, meaning that in neutral water, both concentrations are 1.0 x 10^-7 M.
However, when an acid is added, it increases the concentration of [H+]. Since perchloric acid completely dissociates, the concentration of [H+] is equal to the initial concentration of the acid, which in this case is 0.01 M.
So, [H+] = 0.01 M
Since the concentrations of [H+] and [OH-] in water are inversely proportional, you can use the equilibrium constant expression for water (Kw) to find the concentration of [OH-]:
Kw = [H+] x [OH-]
By rearranging this equation, you can solve for [OH-]:
[OH-] = Kw / [H+]
Substituting the given values:
[OH-] = (1.0 x 10^-7 M^2) / 0.01 M
Simplifying:
[OH-] = 1.0 x 10^-5 M
Therefore, for a 0.01 M perchloric acid solution, the concentration of [H+] is 0.01 M, and the concentration of [OH-] is 1.0 x 10^-5 M.