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
![**Instruction:** Determine the \( pH \) of each of the following solutions.
*Note:* Ensure you have accurate concentration values and any necessary equations at hand to properly calculate the \( pH \). Consider the nature of the solutions (acidic or basic) and make use of the formula \( pH = -\log[H^+] \) for acidic solutions or \( pH = 14 + \log[OH^-] \) for basic ones.
**Context for Students:**
Understanding the \( pH \) scale is crucial, as it measures how acidic or basic a solution is. Solutions with a \( pH \) less than 7 are acidic, greater than 7 are basic, and exactly 7 is neutral.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8bccc44d-7782-46f2-838e-c140c2dedd7b%2F98f6114e-87e9-4997-a316-9227764f6d3b%2Ff76nix_processed.png&w=3840&q=75)
Transcribed Image Text:**Instruction:** Determine the \( pH \) of each of the following solutions.
*Note:* Ensure you have accurate concentration values and any necessary equations at hand to properly calculate the \( pH \). Consider the nature of the solutions (acidic or basic) and make use of the formula \( pH = -\log[H^+] \) for acidic solutions or \( pH = 14 + \log[OH^-] \) for basic ones.
**Context for Students:**
Understanding the \( pH \) scale is crucial, as it measures how acidic or basic a solution is. Solutions with a \( pH \) less than 7 are acidic, greater than 7 are basic, and exactly 7 is neutral.
![### Calculating the pH of a NaCl Solution
**Given:**
- 0.11 M NaCl
**Task:**
Express your answer to two decimal places.
**Instructions:**
1. Calculate the pH of the 0.11 M NaCl solution and enter your answer.
2. Use the equation editor tools as needed:
- The first icon allows you to insert a square root or exponent.
- The second icon provides access to additional symbols and operators.
- Use the undo and redo arrows to correct any mistakes.
- Click the keyboard icon for on-screen typing assistance.
- The question mark offers help if you need further guidance.
**pH Calculation:**
\[ pH = \_\_\_\_ \]
**Additional Notes:**
- NaCl (sodium chloride) is a neutral salt, formed from a strong acid (HCl) and a strong base (NaOH), and it does not affect the pH of the solution.
- Therefore, the pH of the solution is expected to be close to neutral.
Enter your result utilizing the tools provided to ensure accurate formatting and expression.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8bccc44d-7782-46f2-838e-c140c2dedd7b%2F98f6114e-87e9-4997-a316-9227764f6d3b%2Fhaqfy4_processed.png&w=3840&q=75)
Transcribed Image Text:### Calculating the pH of a NaCl Solution
**Given:**
- 0.11 M NaCl
**Task:**
Express your answer to two decimal places.
**Instructions:**
1. Calculate the pH of the 0.11 M NaCl solution and enter your answer.
2. Use the equation editor tools as needed:
- The first icon allows you to insert a square root or exponent.
- The second icon provides access to additional symbols and operators.
- Use the undo and redo arrows to correct any mistakes.
- Click the keyboard icon for on-screen typing assistance.
- The question mark offers help if you need further guidance.
**pH Calculation:**
\[ pH = \_\_\_\_ \]
**Additional Notes:**
- NaCl (sodium chloride) is a neutral salt, formed from a strong acid (HCl) and a strong base (NaOH), and it does not affect the pH of the solution.
- Therefore, the pH of the solution is expected to be close to neutral.
Enter your result utilizing the tools provided to ensure accurate formatting and expression.
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