Quantitative Chemical Analysis
Quantitative Chemical Analysis
9th Edition
ISBN: 9781464135385
Author: Daniel C. Harris
Publisher: W. H. Freeman
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Chapter 6, Problem 6.47P

(a)

Interpretation Introduction

Interpretation:

  • The stepwise acid-base reaction in water for given ions has to be written.
  • The correct symbol for equilibrium constant for this reaction has to be written.

H3N+CH2CH2N+H3

Concept introduction:

Consider a weak-acid equilibrium reaction,

HAKaH++A-

The acid dissociation constant Ka can be given as,

Ka=[H+][A-][HA]

Consider a reaction of weak base,

B+H2OKbBH++OH-

The value of Kb can be calculated as,

Kb=[BH+][OH-][B]

Where Kb is called as base dissociation constant.

The value of Kw is calculated by the formula,

Kw=Ka×Kb

(b)

Interpretation Introduction

Interpretation:

  • The stepwise acid-base reaction in water for given ions has to be written.
  • The correct symbol for equilibrium constant for this reaction has to be written.

-OOCCH2COO-

Concept introduction:

Consider a weak-acid equilibrium reaction,

HAKaH++A-

The acid dissociation constant Ka can be given as,

Ka=[H+][A-][HA]

Consider a reaction of weak base,

B+H2OKbBH++OH-

The value of Kb can be calculated as,

Kb=[BH+][OH-][B]

Where Kb is called as base dissociation constant.

The value of Kw is calculated by the formula,

Kw=Ka×Kb

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General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY