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In a neutral solution;

[H+] = [OH-] = 1x10^-7 M

Since [OH-] greater than [H+], the solution is basic.

In all solutions, whether neutral, or acidic or basic,

Kwater should be satisfied.

Kw = [H+][OH-] = 1x10^-14

Since [OH-] = 100[H+]

Kw = [H+] x 100 [H+] = 1x10^-14

[H+]^2 = 1x10^-14 / 100 = 1x10^-16

[H+] = 1x10^-8 M

Check:

[OH-] = Kw / [H+] = 1x10^-14 / 1x10^-8 = 1x10^-6 which is 100 times greater than 1x10^-8

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Let's assume the solution is Water which is:

HOH, and at equilibrium it is exactly balanced:

H+ + OH-

Now, you are saying that OH is increased by 100% or:

2 X 10 ^ 2

This would make H+ 100 times LESS than OH - or

2 X 10^-2

Therefore, H+ has a value of 2 X 10 ^-2 less in concentration in comparison to OH -

This is the correct answer for Calculate H+ : a solution in which [OH -] is 100 times greater than [H+]?