Explanation Given: Mass of diprotic acid (H 2 A) = 0. 558 g Molar mass of diprotic acid = 255 . 8 g / mol Total volume of the acid = 25 .0 mL Volume of added base = 2 0.0 mL pH = 8 . 25 Calculation: Loss of the second proton is represented by the following reaction: Ca(HA) 2 + Ca(OH) 2 → 2 CaA + 2H 2 O Henderson-Hasselbalch equation for an acidic buffer pH = pK a + log [Conjugate Base] [ Acid] ------ (1) pK a = acid dissociation constant [ Base] = concentration of the conjugate base [Acid] = concentration of the acid Here we have: pH = pK a1 + log [CaA] [Ca(HA) 2 ] ----(2) From Part A , we know that the volume of base needed to reach the first equivalence point = 103.81 ml Total volume = 25 ml acid + (103... Interpretation Introduction c. To determine: The pK a2 value of the diprotic acid after adding 20 .0 mL of base past the first equivalence point

Chemistry: Structure and Properties (2nd Edition)

2nd Edition

ISBN: 9780134293936

Author: Nivaldo J. Tro

Publisher: PEARSON

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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.

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Chapter 17, Problem 138E

Interpretation Introduction

b.

To determine:

The pK_a1 value of the diprotic acid after adding 20.0 ml of base past the first equivalence point

Interpretation Introduction

c.

To determine:

The pK_a2 value of the diprotic acid after adding $20 .0 mL$ of base past the first equivalence point

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Chapter 17, Problem 137E

Chapter 17, Problem 139E

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Chapter 17 Solutions

Chemistry: Structure and Properties (2nd Edition)

Ch. 17 - What is the pH range of human blood? How is human...Ch. 17 - What is a buffer? How does a buffer work? How does...Ch. 17 - What is the common ion effect?Ch. 17 - What is the HendersonHasselbalch equation, and why...Ch. 17 - What is the pH of a buffer when the concentrations...Ch. 17 - Suppose that a buffer contains equal amounts of a...Ch. 17 - How do you use the Henderson—Hasselbalch equation...Ch. 17 - What factors influence the effectiveness of a...Ch. 17 - What is the effective pH range of a buffer...Ch. 17 - Describe acidbase titration. What is the...

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b. To determine: The pK a1 value of the diprotic acid after adding 20.0 ml of base past the first equivalence point

Solution Summary: The author explains how to determine the volume of added base at the first and second equivalence points.

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b.

To determine:

The pK_a1 value of the diprotic acid after adding 20.0 ml of base past the first equivalence point

c.

To determine:

The pK_a2 value of the diprotic acid after adding $20 .0 mL$ of base past the first equivalence point

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Chapter 17 Solutions

b. To determine: The pK a1 value of the diprotic acid after adding 20.0 ml of base past the first equivalence point

Solution Summary: The author explains how to determine the volume of added base at the first and second equivalence points.

Concept explainers

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b. To determine: The pKa1 value of the diprotic acid after adding 20.0 ml of base past the first equivalence point

c. To determine: The pKa2 value of the diprotic acid after adding 20.0 mL of base past the first equivalence point

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Chapter 17 Solutions

b.

To determine:

The pK_a1 value of the diprotic acid after adding 20.0 ml of base past the first equivalence point

c.

To determine:

The pK_a2 value of the diprotic acid after adding $20 .0 mL$ of base past the first equivalence point