Final answer:
A solution with [OH^-] = 1.00 x 10^-7 is considered neutral because it implies that the corresponding [H3O+] is also 1.00 x 10^-7 to satisfy the ionic product of water.
Step-by-step explanation:
When considering whether a solution is acidic, neutral, or basic, we look at the concentration of hydronium ions ([H3O+]) compared to hydroxide ions ([OH−]). To find out if the solution with [OH−] = 1.00 x 10−7 is acidic, neutral, or basic, we can use the relationship between [OH−] and [H3O+]. This relationship is defined by the ionic product of water at 25°C, which is Kw = [H3O+][OH−] = 1.00 x 10−14.
In this case, since [OH−] is given as 1.00 x 10−7, the corresponding [H3O+] must also be 1.00 x 10−7 to satisfy the ionic product of water (Kw). Therefore, with [H3O+] equal to 1.00 x 10−7M, the solution would be classified as neutral.