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7.) The K, of an acid is determined to be 0.00589. What is the pK,.

7.) The K, of an acid is determined to be 0.00589. What is the pK,.

Chemistry
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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### 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.
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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