Final answer:
In an acidic solution, the concentration of hydronium ions ([H₃O+]) is greater than that of hydroxide ions ([OH⁻]). Such a solution has a [H₃O+] greater than 1.0 × 10⁻⁷ M, and consequently a pH less than 7.00 at 25 °C.
Step-by-step explanation:
Yes, in an acidic solution, the concentration of hydronium ions ([H₃O+]) is greater than the concentration of hydroxide ions ([OH⁻]). To be considered acidic, a solution must have a [H₃O+] greater than 1.0 × 10⁻⁷ M at 25 °C, which also means that its pH will be less than 7.00. The autoionization of water at 25 °C yields a product of [H₃O+][OH⁻] that equals 1.0×10⁻ⁱ⁴, so if [H₃O+] is high, [OH⁻] must be low to maintain this constant product.
For example, if we're given [H₃O+] = 2.0 x 10⁻³, we can calculate [OH⁻] using the formula [OH⁻] = 10⁻ⁱ⁴ ÷ [H₃O+], which would result in a [OH⁻] lower than 1.0 × 10⁻⁷ M, confirming the solution's acidity. This condition aligns with the definition of an acidic solution in which [H₃O+] is much higher than [OH⁻].