How much water must added to 300 ml of 0.2 M solution of CH3 COOH for the degree of dissociation

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How much water must added to 300 ml of 0.2 M solution of CH3...

How much water must added to $300 \mathrm{ml}$ of $0.2 \mathrm{M}$ solution of $\mathrm{CH}_{3} \mathrm{COOH}$ for the degree of dissociation of the acid to double? $K_{\mathrm{a}}$ for the acetic acid $=1.8 \times 10^{-5}$. (a) $1200 \mathrm{ml}$ (b) $300 \mathrm{ml}$ (c) $600 \mathrm{ml}$ (d) $900 \mathrm{ml}$

How much water must added to $300 \mathrm{ml}$ of $0.2 \mathrm{M}$ solution of $\mathrm{CH}_{3} \mathrm{COOH}$ for the degree of dissociation of the acid to double? $K_{\mathrm{a}}$ for the acetic acid $=1.8 \times 10^{-5}$.
(a) $1200 \mathrm{ml}$
(b) $300 \mathrm{ml}$
(c) $600 \mathrm{ml}$
(d) $900 \mathrm{ml}$

Key Concepts

Acid Dissociation Constant (Ka)

This is a fundamental equilibrium constant that quantifies the strength of a weak acid by indicating the extent to which it ionizes in solution. It is defined as the ratio of the concentration of the ionized form (products) to the non-ionized form (reactant) at equilibrium, and it remains unchanged with dilution, making it a crucial parameter when analyzing the behavior of weak acids in solution.

Degree of Dissociation (?)

The degree of dissociation represents the fraction of the original acid molecules that dissociate into ions in solution. It is an important concept in weak acid equilibrium because it directly relates to the concentration of hydrogen ions in the solution, and any change in conditions such as dilution affects this fraction even though the inherent acid strength (Ka) remains constant.

Dilution in Weak Acid Equilibria

Dilution alters the concentration of a weak acid in water, which can lead to an increase in the degree of dissociation due to the shift in the equilibrium position. By adding water, the concentrations of all species decrease, but because Ka is constant, the equilibrium adjusts to produce more dissociated ions, thereby increasing the degree of dissociation.

Equilibrium Concentration Relationships

Understanding how the concentrations of the acid, its conjugate base, and hydrogen ions relate to each other through the equilibrium expression is vital when analyzing changes in conditions such as dilution. Adjustments in these concentrations help to explain the observed behavior of weak acids in solutions when water is added, particularly in contexts where the degree of dissociation is manipulated.

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