What are [H+] and [OH-] for 0.01 M perchloric acid
HClO4 is a strong acid;i.e., it ionizes 100%.
HClO4 ==> H^+ + ClO4^-
Therefore, 0.01M HClO4 = 0.01M (H^+). Then (H^+)(OH^-) = Kw = 1E-14
Solve for OH^-
To determine the concentration of [H+] (hydronium ions) and [OH-] (hydroxide ions) in a solution of perchloric acid, we need to know the acidity of the acid.
Perchloric acid (HClO4) is a strong acid, which means it completely dissociates in water to produce H+ and ClO4- ions.
Since the acid is a monoprotic acid (can only donate one proton), the concentration of H+ ions in the solution will be the same as the concentration of perchloric acid. Therefore, in a 0.01 M perchloric acid solution, the concentration of H+ ions ([H+]) would also be 0.01 M.
On the other hand, the concentration of OH- ions ([OH-]) in pure water at 25°C is 1.0 x 10^-7 M, which is known as the Kw value or the self-ionization constant of water. However, perchloric acid is an acidic solution, so the concentration of OH- ions will be much lower than 1.0 x 10^-7 M.
To calculate the exact concentration of OH- ions, we need to know the concentration of H+ ions, as they are related by the autoionization of water:
[H+] x [OH-] = Kw
Since we know the concentration of H+ ions is 0.01 M, we can rearrange the equation:
[OH-] = Kw / [H+]
Substituting the Kw value of 1.0 x 10^-14 M^2 at 25°C, we can calculate the concentration of OH- ions:
[OH-] = (1.0 x 10^-14 M^2) / (0.01 M)
Calculating this, we find that the concentration of OH- ions in the 0.01 M perchloric acid solution is approximately 1.0 x 10^-12 M.