What is the pH, pOH, [H+] and [OH-] for a solution that contains 5.25 x 10^-3 moles of HCl dissolved in 3.25 L of water?
I was gone the day my teacher explained this and I'm completely lost on what to do.
An outline of steps needed to solve the problem would be helpful. Please do not provide the solution, as I would like to solve it for myself first.
M HCl = mols/L solution = ?
M H^+ = M HCl since HCl is a strong acid and ionizes 100%.
pH = -log (H^+)
pH + pOH = pKw = 14 allows you to calculate pOH after you know pH then
pOH = -log(OH^-) gives you OH^-
Alternatively, after you know (H^+), you can use (H^+)(OH^-) = Kw = 1E-14 to solve for OH^-
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