solution of acctic acid contains (1) CII3 COOII, II^+ (2) CII3 COO^-, II3 O^-, CH3 COOH (3) CII3

step 1 Dear students, in problem 11 of chapter 7 we have asked that aqua solution of acidic can 10 dash

Solution of acctic acid contains (1) CII3 COOII, II^+ (2)...

\Lambdaqucous solution of acctic acid contains (1) $\mathrm{CII}_{3} \mathrm{COOII}, \mathrm{II}^{+}$ (2) $\mathrm{CII}_{3} \mathrm{COO}^{-}, \mathrm{II}_{3} \mathrm{O}^{-}, \mathrm{CH}_{3} \mathrm{COOH}$ (3) $\mathrm{CII}_{3} \mathrm{COO}^{-}, \mathrm{II}_{3} \mathrm{O}^{-}, \mathrm{II}^{+}$ (4) $\mathrm{CII}_{3} \mathrm{COOII}, \mathrm{CII}_{3} \mathrm{COO}^{-}, \mathrm{II}^{+}$

\Lambdaqucous solution of acctic acid contains
(1) $\mathrm{CII}_{3} \mathrm{COOII}, \mathrm{II}^{+}$
(2) $\mathrm{CII}_{3} \mathrm{COO}^{-}, \mathrm{II}_{3} \mathrm{O}^{-}, \mathrm{CH}_{3} \mathrm{COOH}$
(3) $\mathrm{CII}_{3} \mathrm{COO}^{-}, \mathrm{II}_{3} \mathrm{O}^{-}, \mathrm{II}^{+}$
(4) $\mathrm{CII}_{3} \mathrm{COOII}, \mathrm{CII}_{3} \mathrm{COO}^{-}, \mathrm{II}^{+}$

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Key Concepts

Conjugate Acid-Base Pairs

The partially dissociated acid and the ions formed in solution represent a conjugate acid-base pair. The undissociated acid acts as the acid, and its corresponding ion (formed after losing a proton) acts as its conjugate base. Recognizing these pairs is crucial in understanding buffering effects and the overall acid-base behavior in aqueous solutions.

Chemical Equilibrium in Aqueous Solutions

When a weak acid dissolves in water, it reaches a state of dynamic chemical equilibrium, meaning that the rate of the forward reaction (acid dissociation) equals the rate of the reverse reaction (reformation of the acid). This equilibrium determines the concentration of the acid, its conjugate base, and hydrogen ions in the solution, which is essential for calculating properties like pH.

Weak Acid Dissociation

Weak acids, when dissolved in water, do not completely ionize. Instead, they establish an equilibrium between the undissociated acid molecules and the ions produced through partial dissociation. This concept is central to understanding the behavior of acids like acetic acid in aqueous solutions, where only a fraction of the acid molecules donate hydrogen ions to form their conjugate base and hydronium ions.

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