The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic base with a 0.10 M solution of a strong monoprotic acid.**Graph Description:**- **Axis Labels:** - The x-axis represents the "Volume of titrant (mL)" ranging from 0.0 to 50.0 mL. - The y-axis shows the pH, ranging from 0.0 to 12.0.- **Curve Characteristics:** - The curve begins with a high pH around 11, indicating a basic solution before any titrant is added. - As the volume of titrant increases, the pH gradually decreases. - There is a sharp decline in pH between approximately 15 mL and 25 mL of titrant, signifying the equivalence point. - Post-equivalence, the pH levels off around 2 as the solution becomes acidic.Data points are plotted at 1 mL increments.**Questions for Consideration:**(a) What is the pH before any titrant has been added? [ ](b) What is the pH at the midpoint of the titration? [ ](c) What is the pH at the equivalence point? [ ](d) What is the value of Kb for the weak base? [ ]

Answer:When weak base is being titrated against a strong acid, then on adding the acid pH slowly starts falling due to formation of buffer which is shown in the titration curve by flat line. At the midpoint of titration, pOH of the the solution becomes equal to pKb. On keep adding the acid, their is sharp decrease in pH of the solution near the equivalence point shown in the titration curve by vertical line.pH before the addition of any acid, has been marked by red circle corresponding to 0.0mL point and that is 11.0.Since, 20mL of 0.1M weak base is being titrated against 0.1M strong acid and both are monoprotic, therefore equivalence point will be 20mL and midpoint of titration is 10mL. pH corresponding to these point is marked in the titration curve.pH at the midpoint of titration is 9.0, therefore pOH at that point will be:When weak base is titrated against strong acid then at the midpoint of titration, value of pOH will be equal to value of pKb, soAlso,

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The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic base with a 0.10 M solution of a strong monoprotic acid. Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the titration? (c) What is the pH at the equivalence point? (d) What is the value of K, for the weak base? 12.0₁ 10.0 8.0 6.0 4.0 2.0 0.0 0.0 10.0 20.0 30.0 Volume of titrant (mL) AAAAAAAAAAAAAA 40.0 50.0

The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic base with a 0.10 M solution of a strong monoprotic acid. Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the titration? (c) What is the pH at the equivalence point? (d) What is the value of K, for the weak base? 12.0₁ 10.0 8.0 6.0 4.0 2.0 0.0 0.0 10.0 20.0 30.0 Volume of titrant (mL) AAAAAAAAAAAAAA 40.0 50.0

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

The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic base with a 0.10 M solution of a strong monoprotic acid.

**Graph Description:**

- **Axis Labels:**
- The x-axis represents the "Volume of titrant (mL)" ranging from 0.0 to 50.0 mL.
- The y-axis shows the pH, ranging from 0.0 to 12.0.

- **Curve Characteristics:**
- The curve begins with a high pH around 11, indicating a basic solution before any titrant is added.
- As the volume of titrant increases, the pH gradually decreases.
- There is a sharp decline in pH between approximately 15 mL and 25 mL of titrant, signifying the equivalence point.
- Post-equivalence, the pH levels off around 2 as the solution becomes acidic.

Data points are plotted at 1 mL increments.

**Questions for Consideration:**

(a) What is the pH before any titrant has been added? [ ]

(b) What is the pH at the midpoint of the titration? [ ]

(c) What is the pH at the equivalence point? [ ]

(d) What is the value of Kb for the weak base? [ ]

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