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The ionic strength of 0.1 M aqueous solution of Fe2(SO4)3 is:
- a)0.1 M
- b)0.65 M
- c)1.3 M
- d)1.5 M
Correct answer is option 'D'. Can you explain this answer?
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Calculation of Ionic Strength of Fe2(SO4)3 Solution
Ionic Strength Formula:
Ionic strength is calculated using the following formula:
I = 1/2 ∑ (mi × zi^2)
Where,
I = Ionic strength
mi = molarity of ith ion
zi = charge on ith ion
Given:
Molarity of Fe2(SO4)3 solution = 0.1 M
Step 1: Dissociation of Fe2(SO4)3
Fe2(SO4)3 → 2 Fe3+ + 3 SO42-
Step 2: Calculation of Molarity of Fe3+ and SO42- ions
Fe2(SO4)3 solution dissociates into two Fe3+ ions and three SO42- ions.
Molarity of Fe3+ ion = 2 × 0.1 = 0.2 M
Molarity of SO42- ion = 3 × 0.1 = 0.3 M
Step 3: Calculation of Ionic Strength
I = 1/2 ∑ (mi × zi^2)
I = 1/2 [ (0.2 × 3^2) + (0.3 × (-2)^2) ]
I = 1.5 M
Therefore, the ionic strength of 0.1 M aqueous solution of Fe2(SO4)3 is 1.5 M.
Ionic Strength Formula:
Ionic strength is calculated using the following formula:
I = 1/2 ∑ (mi × zi^2)
Where,
I = Ionic strength
mi = molarity of ith ion
zi = charge on ith ion
Given:
Molarity of Fe2(SO4)3 solution = 0.1 M
Step 1: Dissociation of Fe2(SO4)3
Fe2(SO4)3 → 2 Fe3+ + 3 SO42-
Step 2: Calculation of Molarity of Fe3+ and SO42- ions
Fe2(SO4)3 solution dissociates into two Fe3+ ions and three SO42- ions.
Molarity of Fe3+ ion = 2 × 0.1 = 0.2 M
Molarity of SO42- ion = 3 × 0.1 = 0.3 M
Step 3: Calculation of Ionic Strength
I = 1/2 ∑ (mi × zi^2)
I = 1/2 [ (0.2 × 3^2) + (0.3 × (-2)^2) ]
I = 1.5 M
Therefore, the ionic strength of 0.1 M aqueous solution of Fe2(SO4)3 is 1.5 M.
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The ionic strength of 0.1 M aqueous solution of Fe2(SO4)3 is:a)0.1 Mb)0.65 Mc)1.3 Md)1.5 MCorrect answer is option 'D'. Can you explain this answer?
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