- log(1 X 10 -9 M H3O)
= 9 pH
======So, obviously not enough hydronium to be acidic, so a basic solution.
-log(3.4 X 10^-5 M)
= 4.4685
14 - 4.4685
= 9.5 pH
-----------
10.0
4.84
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
The solution must be diluted 1000 times to get from a pH of 3 to a pH of 6.
its 7!
pH=8
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
4.84
When a pH level is 7.0, it is defined as 'neutral' at 25°C because at this pH the concentration of H3O+ equals the concentration of OH− in pure water. - Wikipedia
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
The solution must be diluted 1000 times to get from a pH of 3 to a pH of 6.
its 7!
pH=8
-log[1 X 10^-4 M OH(-)] = 4 14 - 4 = 10 pH ----------------
pH = 14 is basic pH = 7 is neutral pH - 1 and 2 are acidic; pH = 1 is more acidic than pH = 2 Therefore a solution at pH 1 has higher concentration of H+ than at pH 14
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
The concentration of H+ or OH-.
The higher the pH, the greater the concentration of Hydroxide (OH-) ions. So, the solution with the pH of 9 is your answer.