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Given that Ka for acetic acid as 1.8x10⁻5 and Kb of NH₄OH as 1.8x10⁻5 at 25oC,predict the nature of aqueous solution of ammonium acetate
- a)Acidic
- b)Basic
- c)Slightly acidic or basic
- d)Neutral
Correct answer is option 'D'. Can you explain this answer?
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Given that Ka for acetic acid as 1.8x105 and Kb of NHOH as 1.8x105 at ...
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Given that Ka for acetic acid as 1.8x105 and Kb of NHOH as 1.8x105 at ...
Explanation:
To determine the nature of the aqueous solution of ammonium acetate, we need to consider the equilibrium reactions of both acetic acid (CH3COOH) and NHOH (ammonium hydroxide) in water.
Equilibrium reaction of acetic acid:
CH3COOH + H2O ⇌ CH3COO- + H3O+
The equilibrium constant for this reaction is given by the acid dissociation constant (Ka), which is defined as the ratio of the concentration of the products (CH3COO- and H3O+) to the concentration of the reactant (CH3COOH).
The given value of Ka for acetic acid is 1.8x105, which indicates that the reaction favors the formation of products (CH3COO- and H3O+) over the reactant (CH3COOH). Therefore, acetic acid is a weak acid.
Equilibrium reaction of ammonium hydroxide:
NH4OH + H2O ⇌ NH4+ + OH-
The equilibrium constant for this reaction is given by the base dissociation constant (Kb), which is defined as the ratio of the concentration of the products (NH4+ and OH-) to the concentration of the reactant (NH4OH).
The given value of Kb for ammonium hydroxide is also 1.8x105, which indicates that the reaction favors the formation of products (NH4+ and OH-) over the reactant (NH4OH). Therefore, ammonium hydroxide is a weak base.
Ammonium acetate:
Ammonium acetate (NH4CH3COO) is formed by the reaction between ammonium hydroxide and acetic acid. Since both acetic acid and ammonium hydroxide are weak acids and bases respectively, the resulting ammonium acetate will undergo hydrolysis in water.
NH4CH3COO + H2O ⇌ NH4+ + CH3COO- + H3O+
The hydrolysis of ammonium acetate produces an equal concentration of H3O+ and OH- ions, resulting in a neutral pH. Therefore, the aqueous solution of ammonium acetate is neutral.
Conclusion:
The nature of the aqueous solution of ammonium acetate is neutral.
To determine the nature of the aqueous solution of ammonium acetate, we need to consider the equilibrium reactions of both acetic acid (CH3COOH) and NHOH (ammonium hydroxide) in water.
Equilibrium reaction of acetic acid:
CH3COOH + H2O ⇌ CH3COO- + H3O+
The equilibrium constant for this reaction is given by the acid dissociation constant (Ka), which is defined as the ratio of the concentration of the products (CH3COO- and H3O+) to the concentration of the reactant (CH3COOH).
The given value of Ka for acetic acid is 1.8x105, which indicates that the reaction favors the formation of products (CH3COO- and H3O+) over the reactant (CH3COOH). Therefore, acetic acid is a weak acid.
Equilibrium reaction of ammonium hydroxide:
NH4OH + H2O ⇌ NH4+ + OH-
The equilibrium constant for this reaction is given by the base dissociation constant (Kb), which is defined as the ratio of the concentration of the products (NH4+ and OH-) to the concentration of the reactant (NH4OH).
The given value of Kb for ammonium hydroxide is also 1.8x105, which indicates that the reaction favors the formation of products (NH4+ and OH-) over the reactant (NH4OH). Therefore, ammonium hydroxide is a weak base.
Ammonium acetate:
Ammonium acetate (NH4CH3COO) is formed by the reaction between ammonium hydroxide and acetic acid. Since both acetic acid and ammonium hydroxide are weak acids and bases respectively, the resulting ammonium acetate will undergo hydrolysis in water.
NH4CH3COO + H2O ⇌ NH4+ + CH3COO- + H3O+
The hydrolysis of ammonium acetate produces an equal concentration of H3O+ and OH- ions, resulting in a neutral pH. Therefore, the aqueous solution of ammonium acetate is neutral.
Conclusion:
The nature of the aqueous solution of ammonium acetate is neutral.
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Given that Ka for acetic acid as 1.8x105 and Kb of NHOH as 1.8x105 at 25oC,predict the nature of aqueous solution of ammonium acetatea)Acidicb)Basicc)Slightly acidic or basicd)NeutralCorrect answer is option 'D'. Can you explain this answer?
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Given that Ka for acetic acid as 1.8x105 and Kb of NHOH as 1.8x105 at 25oC,predict the nature of aqueous solution of ammonium acetatea)Acidicb)Basicc)Slightly acidic or basicd)NeutralCorrect answer is option 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Given that Ka for acetic acid as 1.8x105 and Kb of NHOH as 1.8x105 at 25oC,predict the nature of aqueous solution of ammonium acetatea)Acidicb)Basicc)Slightly acidic or basicd)NeutralCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Given that Ka for acetic acid as 1.8x105 and Kb of NHOH as 1.8x105 at 25oC,predict the nature of aqueous solution of ammonium acetatea)Acidicb)Basicc)Slightly acidic or basicd)NeutralCorrect answer is option 'D'. Can you explain this answer?.
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