In a solution where [H3O+] > [OH-], the solution is

In a solution where [H3O+] > [OH-], the solution is

• A. Neutral
• B. Acidic
• C. Basic
• D. Amphoteric

Answer: (B)

When the hydronium concentration exceeds the hydroxide concentration, the solution has extra protons, so the pH is below 7. At room temperature, neutral water has [H3O+] = [OH−] ≈ 1×10−7 M; any excess of H3O+ lowers the pH, which defines an acidic solution. The product [H3O+][OH−] equals Kw (about 1×10−14 at 25°C), so a higher [H3O+] shifts the balance toward acidity. This matches an acidic description. It wouldn’t be neutral, and it wouldn’t be basic (which would have [OH−] > [H3O+]); amphoteric refers to a substance that can act as either acid or base, not the state of the solution itself.

When the hydronium concentration exceeds the hydroxide concentration, the solution has extra protons, so the pH is below 7. At room temperature, neutral water has [H3O+] = [OH−] ≈ 1×10−7 M; any excess of H3O+ lowers the pH, which defines an acidic solution. The product [H3O+][OH−] equals Kw (about 1×10−14 at 25°C), so a higher [H3O+] shifts the balance toward acidity. This matches an acidic description. It wouldn’t be neutral, and it wouldn’t be basic (which would have [OH−] > [H3O+]); amphoteric refers to a substance that can act as either acid or base, not the state of the solution itself.