Class 12 Exam > Class 12 Questions > A 0. 00 20 m aqueous solution of an ionic com...
Start Learning for Free
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)
- a)3
- b)4 [2009]
- c)1
- d)2
Correct answer is option 'D'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Verified Answer
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl fre...
ΔTf = 0 – (0.00732°) = 0.00732
ΔTf = i × Kf × m
ΔTf = i × Kf × m
Most Upvoted Answer
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl fre...
The freezing point of a solution is determined by the concentration of solute particles in the solution. In this case, the solute particles are the ions from the ionic compound Co(NH3)5(NO2)Cl.
To calculate the freezing point of the solution, we need to know the van't Hoff factor (i), which represents the number of particles that a solute molecule dissociates into in solution.
In this case, Co(NH3)5(NO2)Cl dissociates into Co2+, 5 NH3, NO2-, and Cl-. So the van't Hoff factor (i) is 7.
The freezing point depression (ΔTf) can be calculated using the formula:
ΔTf = i * Kf * m
Where:
ΔTf = freezing point depression
i = van't Hoff factor
Kf = cryoscopic constant of the solvent
m = molality of the solution
Since the solution is aqueous, the Kf value for water is used. The Kf value for water is 1.86 °C/m.
Given that the molality (m) of the solution is 0.020 m, we can calculate the freezing point depression:
ΔTf = 7 * 1.86 °C/m * 0.020 m
ΔTf = 0.2604 °C
Therefore, the freezing point of the 0.020 m aqueous solution of Co(NH3)5(NO2)Cl would be lowered by 0.2604 °C.
To calculate the freezing point of the solution, we need to know the van't Hoff factor (i), which represents the number of particles that a solute molecule dissociates into in solution.
In this case, Co(NH3)5(NO2)Cl dissociates into Co2+, 5 NH3, NO2-, and Cl-. So the van't Hoff factor (i) is 7.
The freezing point depression (ΔTf) can be calculated using the formula:
ΔTf = i * Kf * m
Where:
ΔTf = freezing point depression
i = van't Hoff factor
Kf = cryoscopic constant of the solvent
m = molality of the solution
Since the solution is aqueous, the Kf value for water is used. The Kf value for water is 1.86 °C/m.
Given that the molality (m) of the solution is 0.020 m, we can calculate the freezing point depression:
ΔTf = 7 * 1.86 °C/m * 0.020 m
ΔTf = 0.2604 °C
Therefore, the freezing point of the 0.020 m aqueous solution of Co(NH3)5(NO2)Cl would be lowered by 0.2604 °C.
|
Explore Courses for Class 12 exam
|
|
Similar Class 12 Doubts
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer?
Question Description
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer?.
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer?.
Solutions for A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
Download more important topics, notes, lectures and mock test series for Class 12 Exam by signing up for free.
Here you can find the meaning of A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer?, a detailed solution for A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice A 0. 00 20 m aqueous solution of an ionic compound Co(NH3)5(NO2)Cl freezes at – 0.00732 °C. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be (Kf = – 1.86°C/m)a)3b)4 [2009]c)1d)2Correct answer is option 'D'. Can you explain this answer? tests, examples and also practice Class 12 tests.
|
|
Explore Courses for Class 12 exam
|
|
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup