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The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2 °C.
(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.
Use: Molal elevation constant (Ebullioscopic Constant), Kb = 0.5 K kg mol-1; Boiling point of pure water is 100°C.)
Q. The value of |y| is ___.
(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.
Use: Molal elevation constant (Ebullioscopic Constant), Kb = 0.5 K kg mol-1; Boiling point of pure water is 100°C.)
Q. The value of |y| is ___.
Correct answer is '2.5'. Can you explain this answer?
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Most Upvoted Answer
The boiling point of water in a 0.1 molal silver nitrate solution (sol...
However, I can provide you with the general formula for calculating the boiling point elevation of a solution:
ΔTb = Kb * molality
where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant (which is a characteristic property of the solvent), and molality is the molality of the solute.
For water as the solvent, Kb is approximately 0.512 °C/m.
Assuming the atmospheric pressure is constant, the boiling point of the solution (Tb) can be calculated by adding the boiling point elevation to the boiling point of pure water (100 °C at standard atmospheric pressure):
Tb = 100 °C + ΔTb
Therefore, to calculate the boiling point of a 0.1 molal silver nitrate solution (solution A), we need to know the molal boiling point elevation constant (Kb) for water and the molality of silver nitrate in solution A.
ΔTb = Kb * molality
where ΔTb is the boiling point elevation, Kb is the molal boiling point elevation constant (which is a characteristic property of the solvent), and molality is the molality of the solute.
For water as the solvent, Kb is approximately 0.512 °C/m.
Assuming the atmospheric pressure is constant, the boiling point of the solution (Tb) can be calculated by adding the boiling point elevation to the boiling point of pure water (100 °C at standard atmospheric pressure):
Tb = 100 °C + ΔTb
Therefore, to calculate the boiling point of a 0.1 molal silver nitrate solution (solution A), we need to know the molal boiling point elevation constant (Kb) for water and the molality of silver nitrate in solution A.
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The boiling point of water in a 0.1 molal silver nitrate solution (sol...
Total moles = 0.05 x 3 + 0.05 x 3 = 0.3 moles
molality = 0.3 / 2 = 0.15
ΔTb = 0.15 x 0.5 = 0.075
B.P. of solution B = 100.75
Difference in B.P. of solution A & Solution B = 100.1 - 100.075
= 0.025
= 2.5 x 10-2
= Y = 2.5
Difference in B.P. of solution A & Solution B = 100.1 - 100.075
= 0.025
= 2.5 x 10-2
= Y = 2.5
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The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer?
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The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. 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 The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer?.
The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. 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 The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer?.
Solutions for The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer?, a detailed solution for The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer? has been provided alongside types of The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice The boiling point of water in a 0.1 molal silver nitrate solution (solution A) is x°C. To this solution A, an equal volume of 0.1 molal aqueous barium chloride solution is added to make a new solution B. The difference in the boiling points of water in the two solutions A and B is y × 10-2°C.(Assume: Densities of the solutions A and B are the same as that of water and the soluble salts dissociate completely.Use: Molal elevation constant (Ebullioscopic Constant), Kb= 0.5 K kg mol-1; Boiling point of pure water is 100°C.)Q.The value of |y| is ___.Correct answer is '2.5'. Can you explain this answer? tests, examples and also practice JEE tests.
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