IIT JAM Exam > IIT JAM Questions > The ionic strength of a solution containing 0...
Start Learning for Free
The ionic strength of a solution containing 0.008 M AlCl3 and 0.005 M KCl is
- a)0.134 M
- b)0.053 M
- c)0.106 M
- d)0.086 M
Correct answer is option 'B'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Verified Answer
The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M K...
Most Upvoted Answer
The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M K...
Explanation:
Ionic strength is a measure of the total concentration of ions in a solution and is calculated using the concentrations and charges of the ions present.
Step 1: Calculate the ionic strength of AlCl3
AlCl3 dissociates into Al3+ and 3Cl- ions.
Concentration of Al3+ = 0.008 M
Concentration of Cl- = 3 * 0.008 M = 0.024 M (since each AlCl3 molecule produces 3 Cl- ions)
Ionic strength of AlCl3 = (concentration of Al3+) * (charge of Al3+)2 + (concentration of Cl-) * (charge of Cl-)2
= (0.008 M) * (3)2 + (0.024 M) * (-1)2
= 0.072 M + 0.024 M
= 0.096 M
Step 2: Calculate the ionic strength of KCl
KCl dissociates into K+ and Cl- ions.
Concentration of K+ = 0.005 M
Concentration of Cl- = 0.005 M
Ionic strength of KCl = (concentration of K+) * (charge of K+)2 + (concentration of Cl-) * (charge of Cl-)2
= (0.005 M) * (1)2 + (0.005 M) * (-1)2
= 0.005 M + 0.005 M
= 0.01 M
Step 3: Calculate the total ionic strength of the solution
Total ionic strength = ionic strength of AlCl3 + ionic strength of KCl
= 0.096 M + 0.01 M
= 0.106 M
Therefore, the ionic strength of the solution containing 0.008 M AlCl3 and 0.005 M KCl is 0.106 M. The correct answer is option B.
Ionic strength is a measure of the total concentration of ions in a solution and is calculated using the concentrations and charges of the ions present.
Step 1: Calculate the ionic strength of AlCl3
AlCl3 dissociates into Al3+ and 3Cl- ions.
Concentration of Al3+ = 0.008 M
Concentration of Cl- = 3 * 0.008 M = 0.024 M (since each AlCl3 molecule produces 3 Cl- ions)
Ionic strength of AlCl3 = (concentration of Al3+) * (charge of Al3+)2 + (concentration of Cl-) * (charge of Cl-)2
= (0.008 M) * (3)2 + (0.024 M) * (-1)2
= 0.072 M + 0.024 M
= 0.096 M
Step 2: Calculate the ionic strength of KCl
KCl dissociates into K+ and Cl- ions.
Concentration of K+ = 0.005 M
Concentration of Cl- = 0.005 M
Ionic strength of KCl = (concentration of K+) * (charge of K+)2 + (concentration of Cl-) * (charge of Cl-)2
= (0.005 M) * (1)2 + (0.005 M) * (-1)2
= 0.005 M + 0.005 M
= 0.01 M
Step 3: Calculate the total ionic strength of the solution
Total ionic strength = ionic strength of AlCl3 + ionic strength of KCl
= 0.096 M + 0.01 M
= 0.106 M
Therefore, the ionic strength of the solution containing 0.008 M AlCl3 and 0.005 M KCl is 0.106 M. The correct answer is option B.
|
Explore Courses for IIT JAM exam
|
|
The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer?
Question Description
The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer?.
The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer?.
Solutions for The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for IIT JAM.
Download more important topics, notes, lectures and mock test series for IIT JAM Exam by signing up for free.
Here you can find the meaning of The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer?, a detailed solution for The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? has been provided alongside types of The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice The ionic strength of a solution containing 0.008 M AlCl3and 0.005 M KCl isa)0.134 Mb)0.053 Mc)0.106 Md)0.086 MCorrect answer is option 'B'. Can you explain this answer? tests, examples and also practice IIT JAM tests.
|
|
Explore Courses for IIT JAM 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
|
Follow Us
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup