A solution of a base differs from a solution of an acid in that the solution of a base? A. is able to conduct electricity B. is able to cause an indicator color change C. has a great [H3O+] D. has a great [OH-]

Option D. has a great [OH⁻]

Explanation:

1) Both acids and bases ionize in aqueous solutions so they are able to conduct electricity.

The ions, being charged particles, when flow through the solution are charge carriers, then they conduct electricity.

So, the option A does not state a difference between a solution of a base and a solution of an acid.

2) Both acids and bases are able to cause an indicator color change.

The usufulness of the indicators is that they are able to change of color when the pH changes either from acid to basic or from basic to acid. There are different indicators because none is suitable for the whole range of pH, but the statement B is not how solutions of base and acids differ.

3) The model of Arrhenius for acids and bases states that an acid is a substance that ionizes in water releasing H⁺ ions (this is equivalent to H₃O⁺) and a base is a substance that releases OH⁻ ions in water. Then, acids have a greater concentration of H₃O⁺ (so option C is not true for a solution of a base) and bases have a greater concentraion of OH⁻, making the option D. true.