13) What is the pH of a 0.001 M solution of Ba(OH)2? a) 11.00 b) 3.00 с). 11.13 d) 2.87
13) What is the pH of a 0.001 M solution of Ba(OH)2? a) 11.00 b) 3.00 с). 11.13 d) 2.87
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![**Question 13:** What is the pH of a 0.001 M solution of Ba(OH)₂?
**Options:**
- a) 11.00
- b) 3.00
- c) 11.13
- d) 2.87
**Explanation:**
To determine the pH of a 0.001 M solution of Ba(OH)₂, we first recognize that Ba(OH)₂ is a strong base and dissociates completely in water to produce barium ions (Ba²⁺) and hydroxide ions (OH⁻).
The concentration of OH⁻ ions will be twice the concentration of Ba(OH)₂ because each formula unit of Ba(OH)₂ produces two OH⁻ ions. Therefore, the concentration of OH⁻ ions is 0.002 M.
To find the pOH, use the formula:
\[ \text{pOH} = -\log[\text{OH}^-] \]
\[ \text{pOH} = -\log(0.002) = 2.7 \]
Finally, to find the pH, use the relationship:
\[ \text{pH} + \text{pOH} = 14 \]
\[ \text{pH} = 14 - 2.7 = 11.3 \]
Matching this with the options provided, choice c) 11.13 is the closest approximation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07d00ca0-0430-458f-a009-3ccbf8c49c5a%2F38cc20bc-1465-4097-9561-d17b8847518e%2Fp4rfftk_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 13:** What is the pH of a 0.001 M solution of Ba(OH)₂?
**Options:**
- a) 11.00
- b) 3.00
- c) 11.13
- d) 2.87
**Explanation:**
To determine the pH of a 0.001 M solution of Ba(OH)₂, we first recognize that Ba(OH)₂ is a strong base and dissociates completely in water to produce barium ions (Ba²⁺) and hydroxide ions (OH⁻).
The concentration of OH⁻ ions will be twice the concentration of Ba(OH)₂ because each formula unit of Ba(OH)₂ produces two OH⁻ ions. Therefore, the concentration of OH⁻ ions is 0.002 M.
To find the pOH, use the formula:
\[ \text{pOH} = -\log[\text{OH}^-] \]
\[ \text{pOH} = -\log(0.002) = 2.7 \]
Finally, to find the pH, use the relationship:
\[ \text{pH} + \text{pOH} = 14 \]
\[ \text{pH} = 14 - 2.7 = 11.3 \]
Matching this with the options provided, choice c) 11.13 is the closest approximation.
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