Calculate the concentration of OH⁻ in a solution that contains 3.9 × 10^-4 M H₃O⁺ at 25°C.Identify the solution as acidic,basic,or neutral. A) 2.6 × 10^-11 M, acidic B) 2.6 × 10^-11 M, basic C) 3.9 × 10^-4 M, neutral D) 2.7 × 10^-2 M, basic E) 2.7 × 10^-2 M, acidic

Question

Quizplus · Accepted Answer

The concentration of OH⁻ in the solution can be calculated using the ion product constant of water (Kw) at 25°C, which is 1.0 × 10⁻¹⁴. 
Kw = [H⁺][OH⁻]
Since the solution contains a proton donor (H⁺, from HSBO⁺), it is acidic.
Let x be the concentration of OH⁻, then the concentration of H⁺ can be calculated as:
(3.9 × 10⁻⁴)(x) = 1.0 × 10⁻¹⁴
x = 2.56 × 10⁻¹¹
Therefore, the concentration of OH⁻ is 2.56 × 10⁻¹¹ M, and the solution is acidic. 
The best choice is A.

Calculate the Concentration of OH⁻ in a Solution That Contains