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A 0.063 M solution of a base has a pH of 11.40.

A 0.063 M solution of a base has a pH of 11.40.

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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**Consider the Strength of the Base** - ○ The base is very weak \((K_b < 1 \times 10^{-8})\). - ○ The base is strong \((K_b > 1 \times 10^{-3})\). - ○ The base is moderately weak \((1 \times 10^{-8} < K_b < 1 \times 10^{-3})\). **Explanation** This text discusses the classification of bases according to their base dissociation constant, \(K_b\). It presents three options to consider: 1. **Very Weak Base**: When \(K_b\) is less than \(1 \times 10^{-8}\), the base is categorized as very weak. 2. **Strong Base**: When \(K_b\) is greater than \(1 \times 10^{-3}\), the base is considered strong. 3. **Moderately Weak Base**: This category includes bases with a \(K_b\) value between \(1 \times 10^{-8}\) and \(1 \times 10^{-3}\). Understanding these categories helps in determining the behavior and reactivity of bases in various chemical reactions.
Transcribed Image Text:**Consider the Strength of the Base** - ○ The base is very weak \((K_b < 1 \times 10^{-8})\). - ○ The base is strong \((K_b > 1 \times 10^{-3})\). - ○ The base is moderately weak \((1 \times 10^{-8} < K_b < 1 \times 10^{-3})\). **Explanation** This text discusses the classification of bases according to their base dissociation constant, \(K_b\). It presents three options to consider: 1. **Very Weak Base**: When \(K_b\) is less than \(1 \times 10^{-8}\), the base is categorized as very weak. 2. **Strong Base**: When \(K_b\) is greater than \(1 \times 10^{-3}\), the base is considered strong. 3. **Moderately Weak Base**: This category includes bases with a \(K_b\) value between \(1 \times 10^{-8}\) and \(1 \times 10^{-3}\). Understanding these categories helps in determining the behavior and reactivity of bases in various chemical reactions.
**Description of a Basic Solution** A 0.063 M solution of a base has a pH of 11.40. **Explanation:** - **Concentration**: The solution has a molarity of 0.063 M, indicating the concentration of the base in moles per liter. - **pH Level**: The pH value of 11.40 signifies that the solution is basic, as pH values above 7 indicate a basic or alkaline solution. This information could be used in educational content related to the properties of bases, pH scale understanding, or chemistry calculations involving molarity and pH.
Transcribed Image Text:**Description of a Basic Solution** A 0.063 M solution of a base has a pH of 11.40. **Explanation:** - **Concentration**: The solution has a molarity of 0.063 M, indicating the concentration of the base in moles per liter. - **pH Level**: The pH value of 11.40 signifies that the solution is basic, as pH values above 7 indicate a basic or alkaline solution. This information could be used in educational content related to the properties of bases, pH scale understanding, or chemistry calculations involving molarity and pH.
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