4. Use the following steps to determine how to make 600 mL of a 0.1M acetate buffer, pH 5.0, using 0.1M acetic acid and 0.1M sodium acetate. a. Consider the Henderson-Hasselbalch equation. pH=pKa + log [base] [acid] Using the desired pH (5.0) and pKą of acetic acid, use the Henderson Hasselbach equation to determine a ratio of [base] [acid] required for this buffer. (For example, your answer should look something like this: [base] [acid] = 2.3 Note that this is NOT the ratio you will obtain - it is just an example) b. Given the example above, we can set [acid] = x and [base] =2.3x. Remember that the concentration of acid and base should equal the desired molarity, which 0.1. Based on this, a second equation can be obtained - given the example above, the equation would. be x + 2.3x = 0.1. Use this to solve for x, which represents the concentration of acid. ([acid]), and for [base].
4. Use the following steps to determine how to make 600 mL of a 0.1M acetate buffer, pH 5.0, using 0.1M acetic acid and 0.1M sodium acetate. a. Consider the Henderson-Hasselbalch equation. pH=pKa + log [base] [acid] Using the desired pH (5.0) and pKą of acetic acid, use the Henderson Hasselbach equation to determine a ratio of [base] [acid] required for this buffer. (For example, your answer should look something like this: [base] [acid] = 2.3 Note that this is NOT the ratio you will obtain - it is just an example) b. Given the example above, we can set [acid] = x and [base] =2.3x. Remember that the concentration of acid and base should equal the desired molarity, which 0.1. Based on this, a second equation can be obtained - given the example above, the equation would. be x + 2.3x = 0.1. Use this to solve for x, which represents the concentration of acid. ([acid]), and for [base].
Transcribed Image Text:### How to Make a 0.1M Acetate Buffer Solution
#### Objective:
To create 600 mL of a 0.1M acetate buffer at pH 5.0 using 0.1M acetic acid and 0.1M sodium acetate.
#### Steps to Follow:
**a. Consider the Henderson-Hasselbalch Equation**
\[ \text{pH} = \text{pKa} + \log \left(\frac{[\text{base}]}{[\text{acid}]}\right) \]
- **Purpose:** Use this equation to find the necessary ratio of base to acid.
- **Given:** Desired pH is 5.0. You need to use the pKa of acetic acid.
- **Calculation Example:** Determine the ratio \([\text{base}]/[\text{acid}]\).
\([ \text{base}]/[\text{acid}] = 2.3\) (example value; the actual ratio may differ).
**b. Establishing Equations**
- **Variable Setting:**
- Let \([\text{acid}] = x\)
- \([\text{base}] = 2.3x\) (based on the example ratio)
- **Total Concentration Equation:**
\[
x + 2.3x = 0.1
\]
- **Solve for \(x\):** \(x\) represents the concentration of acetic acid, from which you can also determine the concentration of the base (\([\text{base}]\)).
Make sure to adjust the calculations based on the correct ratio derived from the specific \(\text{pKa}\) and desired pH values.
Transcribed Image Text:**Buffer Preparation using M1V1 = M2V2 Equation**
To determine the volume of 0.1M acetic acid and 0.1M sodium acetate required for creating a buffer, use the equation M1V1 = M2V2.
1. **M1** = 0.1M of acetic acid or 0.1M sodium acetate (stock solution).
2. **V1** = Volume to solve for.
3. **M2** = The concentration of acid or base calculated in step 4b.
4. **V2** = The desired buffer volume, which is 600 mL.
This equation allows you to calculate how much stock solution (V1) is needed to achieve a specific concentration (M2) in a desired final volume (V2).
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![### How to Make a 0.1M Acetate Buffer Solution
#### Objective:
To create 600 mL of a 0.1M acetate buffer at pH 5.0 using 0.1M acetic acid and 0.1M sodium acetate.
#### Steps to Follow:
**a. Consider the Henderson-Hasselbalch Equation**
\[ \text{pH} = \text{pKa} + \log \left(\frac{[\text{base}]}{[\text{acid}]}\right) \]
- **Purpose:** Use this equation to find the necessary ratio of base to acid.
- **Given:** Desired pH is 5.0. You need to use the pKa of acetic acid.
- **Calculation Example:** Determine the ratio \([\text{base}]/[\text{acid}]\).
\([ \text{base}]/[\text{acid}] = 2.3\) (example value; the actual ratio may differ).
**b. Establishing Equations**
- **Variable Setting:**
- Let \([\text{acid}] = x\)
- \([\text{base}] = 2.3x\) (based on the example ratio)
- **Total Concentration Equation:**
\[
x + 2.3x = 0.1
\]
- **Solve for \(x\):** \(x\) represents the concentration of acetic acid, from which you can also determine the concentration of the base (\([\text{base}]\)).
Make sure to adjust the calculations based on the correct ratio derived from the specific \(\text{pKa}\) and desired pH values.](https://content.bartleby.com/qna-images/question/2910e309-4023-42bb-9437-090123672c12/f25567c8-7b77-45fd-9504-375f02603fb8/eacll38_processed.jpeg)
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