What is the concentration of OH ^- in a solution that contains 3.9 * 10^-⁴M H^-? A) 2.6*10^-¹¹M B) 3.9 *10^-⁴M C) 2.7 * 10^-²M D) 1.0 * 10 ^- ¹⁴M

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The correct answer is A because the concentration of OHF1F1F1S1^F1F1F10in a solution that contains 3.9 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10⁴M HF1F1F1S1^F1F1F10 can be calculated using the following equation:[OHF1F1F1S1^F1F1F10^] = Kw/[HF1F1F1S1^F1F1F10]where Kw is the ion product constant for water (1.0 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10¹⁴M). Substituting the given values into the equation, we get:[OHF1F1F1S1^F1F1F10^] = 1.0 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10¹⁴M / 3.9 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10⁴M = 2.6 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10¹¹M

What Is the Concentration of OH - in a Solution

What Is the Concentration of OH ^- in a Solution