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)+...
icon
Related questions
Question
### 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**
Transcribed Image Text:### 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**
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 1 images

Blurred answer
Knowledge Booster
Complexometric Titrations
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Introductory Chemistry For Today
Introductory Chemistry For Today
Chemistry
ISBN:
9781285644561
Author:
Seager
Publisher:
Cengage
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning