The acid used in above titration is a weak diprotic acid. Briefly explain: 1. how you know it’s diprotic from looking at the titration curve and 2. how you know a weak acid. What is the approximate pH of equivalence point 1? Equivalence point 2? Answer (equivalence point 1):___________________Answer (equivalence point 2):___________________ From the curve, estimate the pKa1 and pKa2. Answer (pKa1):________________ Answer (pKa2):_________________ If we used H2C2O4 as the weak diprotic acid, which of the four species, H2C2O4, HC2O41-, C2O42- or OH1-, will be present in the highest concentrations in a solution at the given pH’s below? If you think any of the above are equal, write the two species that are equal as an equivalence (i.e. H2C2O4 = HC2O41-). pH = 5 Answer:____________ pH = 8 Answer:____________ pH = 12 Answer:____________ **Titration Curve for 0.100 L of a Weak Acid by 1.00 M NaOH**This graph presents the titration curve of a weak acid against a strong base, specifically 0.100 L of a weak acid titrated with 1.00 M NaOH. The horizontal axis represents the volume of NaOH added, measured in liters (L). The vertical axis on the left indicates the pH of the solution, while the right vertical axis indicates the log of the concentration of the undissociated weak acid, represented as log[HnA].### Key Features of the Graph:- **Initial pH**: At 0.000 L of NaOH added, the pH is approximately 2, indicating the acidic nature of the solution.- **Buffer Region**: As more NaOH is added, the pH rises gradually. The buffer region is evident between the volumes of approximately 0.005 L and 0.015 L, where the pH changes slowly due to the weak acid partially neutralizing the base.- **Equivalence Point**: The steepest part of the curve, occurring around 0.022 L of NaOH, indicates the equivalence point where equal moles of acid and base have reacted. At this stage, the solution's pH increases sharply.- **Post-Equivalence Region**: Beyond 0.025 L of NaOH, the curve flattens out as excess NaOH dominates, resulting in a high pH of about 12.This graph effectively illustrates the pH change during the titration of a weak acid with a strong base, showcasing the buffer capacity, equivalence point, and behavior beyond the equivalence. Understanding this curve is essential for interpreting titration results and calculating concentrations in acid-base chemistry.

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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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The acid used in above titration is a weak diprotic acid. Briefly explain: 1. how you know it’s diprotic from looking at the titration curve and 2. how you know a weak acid.

What is the approximate pH of equivalence point 1? Equivalence point 2?

Answer (equivalence point 1):___________________

Answer (equivalence point 2):___________________

From the curve, estimate the pK_a1 and pK_a2.

Answer (pK_a1):________________ Answer (pK_a2):_________________

If we used H₂C₂O₄ as the weak diprotic acid, which of the four species, H₂C₂O₄, HC₂O₄^1-, C₂O₄^2- or OH^1-, will be present in the highest concentrations in a solution at the given pH’s below? If you think any of the above are equal, write the two species that are equal as an equivalence (i.e. H₂C₂O₄ = HC₂O₄^1-).

pH = 5 Answer:____________

pH = 8 Answer:____________

pH = 12 Answer:____________

**Titration Curve for 0.100 L of a Weak Acid by 1.00 M NaOH**

This graph presents the titration curve of a weak acid against a strong base, specifically 0.100 L of a weak acid titrated with 1.00 M NaOH. The horizontal axis represents the volume of NaOH added, measured in liters (L). The vertical axis on the left indicates the pH of the solution, while the right vertical axis indicates the log of the concentration of the undissociated weak acid, represented as log[HnA].

### Key Features of the Graph:

- **Initial pH**: At 0.000 L of NaOH added, the pH is approximately 2, indicating the acidic nature of the solution.

- **Buffer Region**: As more NaOH is added, the pH rises gradually. The buffer region is evident between the volumes of approximately 0.005 L and 0.015 L, where the pH changes slowly due to the weak acid partially neutralizing the base.

- **Equivalence Point**: The steepest part of the curve, occurring around 0.022 L of NaOH, indicates the equivalence point where equal moles of acid and base have reacted. At this stage, the solution's pH increases sharply.

- **Post-Equivalence Region**: Beyond 0.025 L of NaOH, the curve flattens out as excess NaOH dominates, resulting in a high pH of about 12.

This graph effectively illustrates the pH change during the titration of a weak acid with a strong base, showcasing the buffer capacity, equivalence point, and behavior beyond the equivalence. Understanding this curve is essential for interpreting titration results and calculating concentrations in acid-base chemistry.

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