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The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:
- a)1/3 mol kg–1
- b)1/2 mol kg–1
- c)2/5 mol kg–1
- d)3/5 mol kg–1
Correct answer is option 'A'. Can you explain this answer?
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The molality of (NH4)2SO4 solution that has the same ionic strength as...
Calculation of Ionic Strength:
Ionic strength is the measure of the concentration of ions in a solution. It is calculated using the formula:
Ionic strength (I) = 1/2 ∑ ci zi^2
Where,
ci = concentration of the ith ion
zi = charge on the ith ion
For 1 mol kg^-1 solution of KCl, the concentration of K+ and Cl- ions is 1 mol kg^-1 each. Therefore,
Ionic strength (I) = 1/2 [ (1 mol kg^-1) (1^2) + (1 mol kg^-1) (1^2) ]
I = 1 mol kg^-1
Calculation of Molality of (NH4)2SO4 solution:
To find the molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg^-1 solution of KCl, we need to first calculate the concentration of ammonium and sulfate ions in the solution.
(NH4)2SO4 dissociates to give 2 NH4+ ions and 1 SO4^2- ion. Therefore, the total concentration of ions in the solution is:
Concentration of ions = 2[NH4+] + [SO4^2-]
Let x be the molality of (NH4)2SO4 solution. Then,
Concentration of NH4+ ions = 2x mol kg^-1
Concentration of SO4^2- ion = x mol kg^-1
Using the formula for ionic strength, we can write:
I = 1/2 [ (2x mol kg^-1) (1^2) + (x mol kg^-1) (2^2) ]
1 = 2x + 2x
x = 1/3 mol kg^-1
Therefore, the molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg^-1 solution of KCl is 1/3 mol kg^-1.
Ionic strength is the measure of the concentration of ions in a solution. It is calculated using the formula:
Ionic strength (I) = 1/2 ∑ ci zi^2
Where,
ci = concentration of the ith ion
zi = charge on the ith ion
For 1 mol kg^-1 solution of KCl, the concentration of K+ and Cl- ions is 1 mol kg^-1 each. Therefore,
Ionic strength (I) = 1/2 [ (1 mol kg^-1) (1^2) + (1 mol kg^-1) (1^2) ]
I = 1 mol kg^-1
Calculation of Molality of (NH4)2SO4 solution:
To find the molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg^-1 solution of KCl, we need to first calculate the concentration of ammonium and sulfate ions in the solution.
(NH4)2SO4 dissociates to give 2 NH4+ ions and 1 SO4^2- ion. Therefore, the total concentration of ions in the solution is:
Concentration of ions = 2[NH4+] + [SO4^2-]
Let x be the molality of (NH4)2SO4 solution. Then,
Concentration of NH4+ ions = 2x mol kg^-1
Concentration of SO4^2- ion = x mol kg^-1
Using the formula for ionic strength, we can write:
I = 1/2 [ (2x mol kg^-1) (1^2) + (x mol kg^-1) (2^2) ]
1 = 2x + 2x
x = 1/3 mol kg^-1
Therefore, the molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg^-1 solution of KCl is 1/3 mol kg^-1.
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The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer?.
The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer?.
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The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer?, a detailed solution for The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer? has been provided alongside types of The molality of (NH4)2SO4 solution that has the same ionic strength as 1 mol kg–1 solution of KCl is:a)1/3 mol kg–1b)1/2 mol kg–1c)2/5 mol kg–1d)3/5 mol kg–1Correct answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
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