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AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.
(Round off to the nearest integer)
[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]
(Round off to the nearest integer)
[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]
Correct answer is '106'. Can you explain this answer?
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AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a ...
The boiling point of a solution depends on the concentration of solute particles in the solution. In this case, AB2 dissociates into A2 and B-, so there are three solute particles (A2, B-, and AB2) in the solution.
A 10.0 molal solution means that there are 10 moles of solute (AB2) per kilogram of solvent (water).
Since AB2 is 10% dissociated, only 10% of the 10 moles of AB2 will dissociate, giving us 1 mole of A2 and 1 mole of B- in the solution.
Therefore, the total number of solute particles in the solution is 1 (A2) + 1 (B-) + 1 (AB2) = 3.
The boiling point elevation of a solution can be calculated using the equation:
ΔTb = Kb * m * i,
where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant for the solvent (water), m is the molality of the solution, and i is the van't Hoff factor (the number of particles into which the solute dissociates).
We need to find the boiling point elevation, so we can rearrange the equation to solve for ΔTb:
ΔTb = Kb * m * i.
Assuming we have the value for Kb for water, we can plug in the values:
ΔTb = Kb * 10.0 molal * 3.
The boiling point elevation will depend on the specific value of Kb for water, which can be found in a reference table.
Therefore, without the specific value of Kb for water, we cannot determine the boiling point of the 10.0 molal aqueous solution of AB2.
A 10.0 molal solution means that there are 10 moles of solute (AB2) per kilogram of solvent (water).
Since AB2 is 10% dissociated, only 10% of the 10 moles of AB2 will dissociate, giving us 1 mole of A2 and 1 mole of B- in the solution.
Therefore, the total number of solute particles in the solution is 1 (A2) + 1 (B-) + 1 (AB2) = 3.
The boiling point elevation of a solution can be calculated using the equation:
ΔTb = Kb * m * i,
where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant for the solvent (water), m is the molality of the solution, and i is the van't Hoff factor (the number of particles into which the solute dissociates).
We need to find the boiling point elevation, so we can rearrange the equation to solve for ΔTb:
ΔTb = Kb * m * i.
Assuming we have the value for Kb for water, we can plug in the values:
ΔTb = Kb * 10.0 molal * 3.
The boiling point elevation will depend on the specific value of Kb for water, which can be found in a reference table.
Therefore, without the specific value of Kb for water, we cannot determine the boiling point of the 10.0 molal aqueous solution of AB2.
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AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a ...
AB2 ⇌ A+ + 2B-
∴ For AB2, n = 3
i = 1 + (n - 1)α
= 1 + (3 - 1) x 0.1
= 1.12
Now, ΔTb = Kb(im)
∴ For AB2, n = 3
i = 1 + (n - 1)α
= 1 + (3 - 1) x 0.1
= 1.12
Now, ΔTb = Kb(im)
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AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer?
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AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer?.
AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer?.
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AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer?, a detailed solution for AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer? has been provided alongside types of AB2 is 10% dissociated in water to A2+ and B-. The boiling point of a 10.0 molal aqueous solution of AB2 is ________°C.(Round off to the nearest integer)[Given: Molal elevation constant of water, Kb = 0.5 K kg mol-1; boiling point of pure water = 100°C]Correct answer is '106'. Can you explain this answer? theory, EduRev gives you an
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