Given an OH^- concentration of 1.0 × 10^-6 M, calculate the H₃O⁺ concentration, and then identify the solution as acidic, basic, or neutral. A)[H₃O⁺] = 1.0 × 10^-7, neutral B)[H₃O⁺] = 1.0 × 10^-6, acidic C)[H₃O⁺] = 1.0 × 10^-8, acidic D)[H₃O⁺] = 1.0 × 10^-8, basic E)[H₃O⁺] = 1.0 × 10^-6, basic

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Quizplus · Accepted Answer

Given the concentration of OH^- (hydroxide ions) is 1.0 × 10^-6 M, the solution is basic because OH^- is a base. The concentration of H3O^+ (hydronium ions) can be found using the water dissociation constant (Kw = 1.0 × 10^-14 at 25°C), where [H3O^+][OH^-] = Kw. Thus, [H3O^+] = Kw / [OH^-] = 1.0 × 10^-14 / 1.0 × 10^-6 = 1.0 × 10^-8 M, indicating a basic solution due to the lower concentration of H3O^+ compared to OH^-.

Given an OH- Concentration of 1

Given an OH^- Concentration of 1