Determine whether the following hydroxide ion concentrations ([OH−]) correspond to acidic, basic, or neutral solutions by estimating their corresponding hydronium ion concentrations ([H3O+] using the ion product constant of water (Kw). Hydronium ion concentration [H3O+] Solution condition Greater than 1×10−7 M Acidic Equal to 1×10−7 M Neutral Less than 1×10−7 M Basic It may help to keep the following equation in mind as you work Kw = [H3O+][OH−] = [1×10−7 M][1×10−7 M] = 1×10−14 M Drag the appropriate items to their respective bins.

See explanation below

Explanation:

The question is incomplete. However, I managed to find a similar question with these values of [OH⁻]. If these values are not the same that you have, don't worry, you all need to replace your given data in this procedure, and you should get the accurate results. The concentrations here will be:

[OH-]=10x10^-12M

[OH-]=7x10^-9M

[OH-]=7x10^-4M

[OH-]=8X10^-10M

[OH-]=1X10^-5M

[OH-]=4X10^-13M

[OH-]=1X10^-7M

[OH-]=2X10^-2

Now, to get the [H₃O⁺] we just use the following expression:

Kw = [OH⁻] [H₃O⁺] > [H₃O⁺] = Kw / [OH⁻]

Applying this expression, we'll get the hydronium concentrations and then, we could see which one is acidic, basic or neutral:

a) [OH-] = 1x10⁻¹² M

[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻¹² = 0.01 M or 1x10⁻² M. Acidic

b) [OH-]= 7x10⁻⁹ M

[H₃O⁺] = 1x10⁻¹⁴ / 7x10⁻⁹ = 1.43x10⁻⁶ M. Acidic

c) [OH-] = 7x10⁻⁴ M

[H₃O⁺] = 1x10⁻¹⁴ / 7x10⁻⁴ = 1.43x10⁻¹¹ M. Basic

d) [OH-] = 8x10⁻¹⁰M

[H₃O⁺] = 1x10⁻¹⁴ / 8x10⁻¹⁰ = 1.25x10⁻⁵ M. Acidic

e) [OH-] = 1x10⁻⁵M

[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻⁵ = 1x10⁻⁹ M. Basic.

f) [OH-] = 4x10⁻¹³ M

[H₃O⁺] = 1x10⁻¹⁴ / 4x10⁻¹³ = 2.5x10⁻² M. Acidic

g) [OH-] = 1x10⁻⁷ M

[H₃O⁺] = 1x10⁻¹⁴ / 1x10⁻⁷ = 1x10⁻⁷ M. Neutral

h) [OH-] = 2x10⁻² M

[H₃O⁺] = 1x10⁻¹⁴ / 2x10⁻² = 5x10⁻¹³ M. Basic.

i think it's c. i'm not sure but i think so.