What relationship exists between H^+ ion concentration and OH^- ion concentration? Waht is the OH^- concentration of an aqueous solution with the H^+ concentration of 10^-4M. Calculate the pOH? Need help with this pls. thank you.
(H^+)(OH^-) = Kw = 1E-14
The relationship between H^+ ion concentration and OH^- ion concentration is based on the concept of pH and pOH. In an aqueous solution, water molecules can dissociate into H^+ ions (or H3O^+ ions) and OH^- ions through the process of self-ionization:
2H2O ⇌ H3O^+ + OH^-
In pure water, at 25 degrees Celsius, the concentration of H^+ ions and OH^- ions is 10^-7 M. This is because the self-ionization of water is a reversible reaction, and in pure water, the concentration of H^+ ions and OH^- ions is equal and very low.
Now let's consider your specific question: Given an H^+ ion concentration of 10^-4 M, we can determine the OH^- concentration and pOH using the following formulas:
pOH = -log[OH^-]
OH^- = Kw / [H^+]
where Kw is the ionization constant of water, which is equal to 1.0 x 10^-14 at 25 degrees Celsius.
To find the OH^- concentration, we can substitute the H^+ concentration into the equation OH^- = Kw / [H^+]:
OH^- = (1.0 x 10^-14) / (10^-4)
OH^- = 1.0 x 10^-10 M
So, the OH^- concentration of the aqueous solution with an H^+ concentration of 10^-4 M is 1.0 x 10^-10 M.
To calculate the pOH, we use the formula pOH = -log[OH^-]:
pOH = -log(1.0 x 10^-10)
pOH = 10
Therefore, the pOH of the aqueous solution is 10.
I hope this explanation helps! Let me know if you have any further questions.