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Convert a pH value of 3.7 to [OH-].

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pH = -log[H+]

Therefore, [H+] = 10^(-pH)
= 10^(-3.7)
= 2.01 x 10^(-4) M

Since water dissociates into equal parts of [H+] and [OH-], we can calculate [OH-] using the equation Kw = [H+][OH-] and solve for [OH-]:

Kw = 1.0 x 10^(-14)

[OH-] = Kw / [H+]
= (1.0 x 10^(-14)) / (2.01 x 10^(-4))
= 4.98 x 10^(-11) M

Therefore, the concentration of hydroxide ions in a solution with a pH of 3.7 is 4.98 x 10^(-11) M.
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