2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A commonly seen definition of buffer capacity is: "The amount of H* or OH that can be neutralized before the pH changes to a significant degree." Use your data to determine the buffer capacity of Buffer A and Buffer B. 3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC₂H3O2, with 100.0 mL of 1.0 M acetic acid. a. What would be the initial pH of Buffer C? b. If you add 5.0 mL of 0.5 M NaOH solution to 20.0 ml. affer B
2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A commonly seen definition of buffer capacity is: "The amount of H* or OH that can be neutralized before the pH changes to a significant degree." Use your data to determine the buffer capacity of Buffer A and Buffer B. 3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC₂H3O2, with 100.0 mL of 1.0 M acetic acid. a. What would be the initial pH of Buffer C? b. If you add 5.0 mL of 0.5 M NaOH solution to 20.0 ml. affer B
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Chapter1: Chemical Foundations
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Question
Hello can you help me answer question 2,3.a, and 3.b please? Thank you!
![**DATA ANALYSIS**
1. Write reaction equations to explain how your acetic acid-acetate buffer reacts with a base.
2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A buffer capacity is the amount of \[H^+\] or \[OH^-\] that can be neutralized before the pH changes significantly. Use your data to determine the buffer capacity of Buffer A and Buffer B.
3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.00 M acetic acid.
a. What would be the initial pH of Buffer C?
b. If you add mL of 0.5 M NaOH solution to 20.0 mL each of Buffer B and Buffer C, which buffer's pH would change less? Explain.
**DATA TABLE**
| Mass of NaC2H3O2 used to prepare buffer (g) | Volume of buffer prepared (mL) | Molar concentration of HCl/Na2O2 buffer (M) | Initial pH of buffer | Volume of 0.5 M HCl to lower pH by 2 units (mL) | Volume of 0.5 M NaOH to raise pH by 2 units (mL) | Volume of 0.5 M NaOH at equivalence point (mL) |
|---------------------------------------------|--------------------------------|---------------------------------------------|----------------------|-------------------------------------------------|--------------------------------------------------|-----------------------------------------------|
| Buffer A | 0.15139 | 100.0 | 1.5 mL | 4.79 | 1.0 mL | 1.5 mL |
| Buffer B | 1.50018 | 100.0 | 10 | 4.73 | 1.9 mL | 2 mL | 4.5 mL | 90 mL |
The above table provides detailed data regarding the preparation and characterization of two different buffers, Buffer A and Buffer B, including their initial pH levels and their reactions with acid and base solutions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9fdad347-f735-4012-90dd-d6f7d68bdff1%2Fa6fb7547-498e-48fd-8661-864c1b4fe661%2F4s8c40t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**DATA ANALYSIS**
1. Write reaction equations to explain how your acetic acid-acetate buffer reacts with a base.
2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A buffer capacity is the amount of \[H^+\] or \[OH^-\] that can be neutralized before the pH changes significantly. Use your data to determine the buffer capacity of Buffer A and Buffer B.
3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.00 M acetic acid.
a. What would be the initial pH of Buffer C?
b. If you add mL of 0.5 M NaOH solution to 20.0 mL each of Buffer B and Buffer C, which buffer's pH would change less? Explain.
**DATA TABLE**
| Mass of NaC2H3O2 used to prepare buffer (g) | Volume of buffer prepared (mL) | Molar concentration of HCl/Na2O2 buffer (M) | Initial pH of buffer | Volume of 0.5 M HCl to lower pH by 2 units (mL) | Volume of 0.5 M NaOH to raise pH by 2 units (mL) | Volume of 0.5 M NaOH at equivalence point (mL) |
|---------------------------------------------|--------------------------------|---------------------------------------------|----------------------|-------------------------------------------------|--------------------------------------------------|-----------------------------------------------|
| Buffer A | 0.15139 | 100.0 | 1.5 mL | 4.79 | 1.0 mL | 1.5 mL |
| Buffer B | 1.50018 | 100.0 | 10 | 4.73 | 1.9 mL | 2 mL | 4.5 mL | 90 mL |
The above table provides detailed data regarding the preparation and characterization of two different buffers, Buffer A and Buffer B, including their initial pH levels and their reactions with acid and base solutions.
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