### Question: What is the hydronium-ion concentration of a 0.0038 M Ba(OH)₂ solution?### Options:- A) 1.3 × 10⁻¹² M- B) 7.6 × 10⁻³ M- C) 1.0 × 10⁻⁷ M- D) 3.8 × 10⁻³ M- E) 2.6 × 10⁻¹² M### Explanation:In this problem, we need to determine the concentration of hydronium ions (H₃O⁺) in a given solution of barium hydroxide, Ba(OH)₂. Remember, Ba(OH)₂ is a strong base and completely dissociates in an aqueous solution as follows:\[ \text{Ba(OH)₂} \rightarrow \text{Ba}^{2+} + 2\text{OH}^- \]For a 0.0038 M Ba(OH)₂ solution:1. The concentration of OH⁻ ions will be twice the concentration of Ba(OH)₂ because one Ba(OH)₂ produces two OH⁻ ions upon dissociation. \[ \text{[OH]⁻} = 2 \times 0.0038 \, M = 0.0076 \, M \]Using the water dissociation constant: \[ K_w = [H₃O⁺][OH]⁻ = 1.0 \times 10^{-14} \, M^{2}\]We can find the concentration of H₃O⁺: \[ [H₃O⁺] = \frac{1.0 \times 10^{-14}}{0.0076} \approx 1.3 \times 10^{-12} \, M \]Therefore, the correct answer is:- **A) 1.3 × 10⁻¹² M**

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What is the hydronium-ion concentration of a 0.0038 M Ba(OH)2 solution? 1.3 x 10-12 M O 7.6 x 10-3 M O 1.0 x 10-7 M O 3.8 x 10-3 M O 2.6 x 10-12 M

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 60QAP: Consider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+...

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