-log[1 X 10^-4 M OH(-)]
= 4
14 - 4
= 10 pH
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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
Yes, if both solutions are at 25oC then in both solutions this is valid: pH + pOH = 14.0
Molarity of hydrogen solution equals 2.3 X 10^-4 -log(2.3 X 10^-4) = 3.6 pH
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
2
The solution must be diluted 1000 times to get from a pH of 3 to a pH of 6.
its 7!
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
When diluted 10 times pH is raised by 1 unit in a acid.So you have to dilute 1000 times.
1 x 104
100,000 times more acidic
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
Yes, if both solutions are at 25oC then in both solutions this is valid: pH + pOH = 14.0
Molarity of hydrogen solution equals 2.3 X 10^-4 -log(2.3 X 10^-4) = 3.6 pH
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
1.15
6.15