Given an OH⁻ concentration of 1.0 × 10⁻⁴ 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^-4, acidic C)[H₃O⁺] = 1.0 × 10^-10, acidic D)[H₃O⁺] = 1.0 × 10^-10, basic E)[H₃O⁺] = 1.0 × 10^-4, basic

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Quizplus · Accepted Answer

Given the concentration of $[OH^-] = 1.0 \times 10^{-4} M$, this indicates a basic solution because the concentration of hydroxide ions is higher than $1.0 \times 10^{-7} M$, which is the concentration of hydroxide ions in neutral water at 25°C. To find the concentration of $[H_3O^+]$, we use the water dissociation constant $K_w = 1.0 \times 10^{-14}$ at 25°C, where $K_w = [H_3O^+][OH^-]$. Substituting the given $[OH^-]$ into the equation gives $[H_3O^+] = \frac{1.0 \times 10^{-14}}{1.0 \times 10^{-4}} = 1.0 \times 10^{-10} M$. This low concentration of hydronium ions compared to the neutral concentration of $1.0 \times 10^{-7} M$ confirms the solution is basic.

Given an OH− Concentration of 1

Given an OH⁻ Concentration of 1