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The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is?
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The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3...
Solution:
Introduction
In chemistry, hydrolysis is a chemical reaction between water and another substance to form two or more new substances. The hydrolysis constant of a salt is the equilibrium constant for the reaction of the salt with water to produce the corresponding acid and base. Ammonium chloride is an example of a salt that undergoes hydrolysis.
Given
Hydrolysis constant of NH4Cl = 5.6×10^-10
Concentration of NH4Cl = 0.1 M
Formula
The hydrolysis constant expression for NH4Cl is given as follows:
NH4Cl + H2O ⇌ NH4+ + Cl- + H3O+
Kw = [NH4+][Cl-]/[NH4Cl]
Ka = [NH4+][H3O+]/[NH4Cl]
Kb = [NH3][OH-]/[NH4+]
Kw = Ka * Kb
pH = -log[H3O+]
Calculation
From the given hydrolysis constant expression, we can find the concentration of H3O+ by using the formula for Ka:
Ka = [NH4+][H3O+]/[NH4Cl]
Let x be the concentration of H3O+ produced by the hydrolysis of NH4Cl. Then, the concentration of NH4+ and Cl- can be written as (0.1 - x). Therefore, the expression for Ka becomes:
Ka = x^2 / (0.1 - x)
Using the hydrolysis constant of NH4Cl, we can find the concentration of OH- produced by the reaction of NH4+ with water:
Kb = [NH3][OH-]/[NH4+]
Kb = Kw / Ka = (1.0 * 10^-14) / (5.6 * 10^-10) = 1.8 * 10^-5
[NH3] = [OH-] = sqrt(Kb * [NH4+]) = sqrt(1.8 * 10^-5 * (0.1 - x))
The concentration of H3O+ can be calculated using the formula for pH:
pH = -log[H3O+]
[H3O+] = 10^-pH
Answer
The concentration of H3O+ in a 0.1M solution of NH4Cl at equilibrium is 4.74 * 10^-6 M.
Explanation
The hydrolysis of NH4Cl produces NH4+ and Cl- ions, which react with water to produce H3O+ and OH- ions. The equilibrium constant expression for this reaction is given by Kw = [NH4+][Cl-]/[NH4Cl]. The hydrolysis constant expression for NH4Cl is Ka = [NH4+][H3O+]/[NH4Cl]. We can use this expression to find the concentration of H3O+ produced by the hydrolysis of NH4Cl. By using the hydrolysis constant of NH4Cl, we can also find the concentration of OH- produced by the reaction of NH4+ with water. Finally, we can use the formula for pH to calculate the concentration of H3
Introduction
In chemistry, hydrolysis is a chemical reaction between water and another substance to form two or more new substances. The hydrolysis constant of a salt is the equilibrium constant for the reaction of the salt with water to produce the corresponding acid and base. Ammonium chloride is an example of a salt that undergoes hydrolysis.
Given
Hydrolysis constant of NH4Cl = 5.6×10^-10
Concentration of NH4Cl = 0.1 M
Formula
The hydrolysis constant expression for NH4Cl is given as follows:
NH4Cl + H2O ⇌ NH4+ + Cl- + H3O+
Kw = [NH4+][Cl-]/[NH4Cl]
Ka = [NH4+][H3O+]/[NH4Cl]
Kb = [NH3][OH-]/[NH4+]
Kw = Ka * Kb
pH = -log[H3O+]
Calculation
From the given hydrolysis constant expression, we can find the concentration of H3O+ by using the formula for Ka:
Ka = [NH4+][H3O+]/[NH4Cl]
Let x be the concentration of H3O+ produced by the hydrolysis of NH4Cl. Then, the concentration of NH4+ and Cl- can be written as (0.1 - x). Therefore, the expression for Ka becomes:
Ka = x^2 / (0.1 - x)
Using the hydrolysis constant of NH4Cl, we can find the concentration of OH- produced by the reaction of NH4+ with water:
Kb = [NH3][OH-]/[NH4+]
Kb = Kw / Ka = (1.0 * 10^-14) / (5.6 * 10^-10) = 1.8 * 10^-5
[NH3] = [OH-] = sqrt(Kb * [NH4+]) = sqrt(1.8 * 10^-5 * (0.1 - x))
The concentration of H3O+ can be calculated using the formula for pH:
pH = -log[H3O+]
[H3O+] = 10^-pH
Answer
The concentration of H3O+ in a 0.1M solution of NH4Cl at equilibrium is 4.74 * 10^-6 M.
Explanation
The hydrolysis of NH4Cl produces NH4+ and Cl- ions, which react with water to produce H3O+ and OH- ions. The equilibrium constant expression for this reaction is given by Kw = [NH4+][Cl-]/[NH4Cl]. The hydrolysis constant expression for NH4Cl is Ka = [NH4+][H3O+]/[NH4Cl]. We can use this expression to find the concentration of H3O+ produced by the hydrolysis of NH4Cl. By using the hydrolysis constant of NH4Cl, we can also find the concentration of OH- produced by the reaction of NH4+ with water. Finally, we can use the formula for pH to calculate the concentration of H3
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The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3...
The hydrolysis constant of NH4Cl is 5.6×10-10 . the concentration of h3o+in a 0.1M solution of NH4Cl is
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The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is?
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The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is? for GATE 2025 is part of GATE preparation. The Question and answers have been prepared according to the GATE exam syllabus. Information about The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is? covers all topics & solutions for GATE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is?.
The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is? for GATE 2025 is part of GATE preparation. The Question and answers have been prepared according to the GATE exam syllabus. Information about The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is? covers all topics & solutions for GATE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The hydrolysis constant of NH4Cl is 5.6×10-10 .the concentration of h3o in a 0.1M solution of NH4Cl at equlibrium is?.
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