### Titration of a Mixture of Two Weak Acids#### Experimental SetupYou are provided with a solution containing a mixture of two weak acids. A 50.00 mL sample of this mixture is titrated with 0.1000 M NaOH using a pH meter. The data collected is presented in the graph below.#### Graph Explanation**Title:** Titration of a Mixture- **X-axis:** Volume of NaOH added (mL)- **Y-axis:** pHThe graph shows a titration curve where the pH of the solution is plotted against the volume of NaOH added. Initially, the pH rises gradually. Two distinct buffer regions with steeper rises indicate the presence of two weak acids. - **First Equivalence Point:** The initial steep increase around 10 mL indicates the first equivalence point, where the first acid is neutralized.- **Second Equivalence Point:** Another rapid increase around 25 mL indicates the second equivalence point, corresponding to the neutralization of the second acid.#### Analysis Task1. **Determine the Equivalence Volumes:** - Identify the volume at each equivalence point from the titration curve.2. **Calculate Moles of NaOH:** - Use the equivalence volumes to calculate the moles of NaOH used at each step with the formula: moles = volume (L) × concentration (M).3. **Determine Concentrations of Acids:** - Calculate the concentrations of each acid in the original mixture using the moles of NaOH.4. **Estimate pKa Values:** - Analyze the titration curve to estimate the pKa values of each acid. This can be observed at the midpoint of each buffer region (half-equivalence point).5. **Documentation:** - Show calculations and justify choices with explanations.This exercise provides insight into the titration process of mixed weak acids, using pH changes to determine various properties of the acids present.

Volume of sample = 50.00 mL Molarity of NaOH = 0.1000 M

You are given a solution that contains a mixture of two weak acids. You take a 50.00 mL sample of the mixture and titrate it with 0.1000M NaOH using a pH meter. You obtain the data shown in the plot below. 12 10 8 6 4 2 0 0 5 Titration of a mixture 10 15 vol (mL) NaOH added 20 25 30 Determine the first and second equivalence volumes. Use the equivalence volumes to determine how many moles of NaOH was used to titrate each acid. Use those values to determine the concentration of each acid in the original mixture. Finally, estimate the pKa values for each acid from the plot. Show your calculations and explain any choices you have made.

You are given a solution that contains a mixture of two weak acids. You take a 50.00 mL sample of the mixture and titrate it with 0.1000M NaOH using a pH meter. You obtain the data shown in the plot below. 12 10 8 6 4 2 0 0 5 Titration of a mixture 10 15 vol (mL) NaOH added 20 25 30 Determine the first and second equivalence volumes. Use the equivalence volumes to determine how many moles of NaOH was used to titrate each acid. Use those values to determine the concentration of each acid in the original mixture. Finally, estimate the pKa values for each acid from the plot. Show your calculations and explain any choices you have made.

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

### Titration of a Mixture of Two Weak Acids

#### Experimental Setup

You are provided with a solution containing a mixture of two weak acids. A 50.00 mL sample of this mixture is titrated with 0.1000 M NaOH using a pH meter. The data collected is presented in the graph below.

#### Graph Explanation

**Title:** Titration of a Mixture

- **X-axis:** Volume of NaOH added (mL)
- **Y-axis:** pH

The graph shows a titration curve where the pH of the solution is plotted against the volume of NaOH added. Initially, the pH rises gradually. Two distinct buffer regions with steeper rises indicate the presence of two weak acids.

- **First Equivalence Point:** The initial steep increase around 10 mL indicates the first equivalence point, where the first acid is neutralized.
- **Second Equivalence Point:** Another rapid increase around 25 mL indicates the second equivalence point, corresponding to the neutralization of the second acid.

#### Analysis Task

1. **Determine the Equivalence Volumes:**
- Identify the volume at each equivalence point from the titration curve.

2. **Calculate Moles of NaOH:**
- Use the equivalence volumes to calculate the moles of NaOH used at each step with the formula: moles = volume (L) × concentration (M).

3. **Determine Concentrations of Acids:**
- Calculate the concentrations of each acid in the original mixture using the moles of NaOH.

4. **Estimate pKa Values:**
- Analyze the titration curve to estimate the pKa values of each acid. This can be observed at the midpoint of each buffer region (half-equivalence point).

5. **Documentation:**
- Show calculations and justify choices with explanations.

This exercise provides insight into the titration process of mixed weak acids, using pH changes to determine various properties of the acids present.

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