Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question 7:** The \( K_a \) of an acid is determined to be 0.00589. What is the \( pK_a \)?
#### Explanation
The \( K_a \) value of an acid is a measure of its acid dissociation constant, which indicates the strength of the acid in solution. To find the \( pK_a \), which is the negative logarithm (base 10) of the \( K_a \), use the formula:
\[ pK_a = -\log_{10}(K_a) \]
By calculating this, you can determine the \( pK_a \) value, which provides insight into the acidity of the compound. A lower \( pK_a \) value corresponds to a stronger acid.
This type of calculation is commonly used in chemistry to compare the strengths of different acids.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fce641f86-6059-4a1b-9ac7-4d71ededb3ba%2F1927baf4-2207-4374-bd03-222ed4305ecf%2Fxzocfgk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Transcription for Educational Content
**Question 7:** The \( K_a \) of an acid is determined to be 0.00589. What is the \( pK_a \)?
#### Explanation
The \( K_a \) value of an acid is a measure of its acid dissociation constant, which indicates the strength of the acid in solution. To find the \( pK_a \), which is the negative logarithm (base 10) of the \( K_a \), use the formula:
\[ pK_a = -\log_{10}(K_a) \]
By calculating this, you can determine the \( pK_a \) value, which provides insight into the acidity of the compound. A lower \( pK_a \) value corresponds to a stronger acid.
This type of calculation is commonly used in chemistry to compare the strengths of different acids.
Expert Solution

Step 1 dissociation constant
PKa = -log(Ka)
This is the relation between Ka and pKa is
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