Which of the following solutions has higher freezing point? 0.05 M Al2(SO4 )3 , 0.1 M K3 [Fe(CN)6 ] Justify.

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Please find below the solution of your asked query:

Reaction Involved-

Al2SO43  2Al3+ + 3SO42-

Number of particles/ions formed after dissociation in Al2(SO4)3 are 5

Reaction Involved-

K3FeCN6  3K+ + FeCN63-

Number of particles/ions formed after dissociation in K3[Fe(CN)6] are 4

So, as number of particles/ions are more in Aluminium sulphate as compared to Potassium hexacyanoferrate (III). Thus, there is higher in deep in freezing point of former. So, ‚ÄčK3[Fe(CN)6] has higher freezing point.

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  • -3
The correct answer is - 0.05 M Al₂(SO₄)₃ has a higher freezing point.

Al₂(SO₄)₃ dissociates in water to give 5 mol of ions per mole of the compound.


The freezing point can be calculated using the formula - ΔTf = i * X, where i is the number of ions formed and X is the concentration.



So, ΔTf of 0.05 M Al₂(SO₄)₃ = 5 x 0.05 = 0.25 moles of ions



Similarly, for K₃[Fe(CN)₆], the number of ions formed on dissociation in water per mole of compound is, i = 4



ΔTf  of K₃[Fe(CN)₆] = 4 x 0.1 = 0.4 moles of ions



Since the Freezing point is directly proportional to the number of dissolved particles, it can be concluded that 0.05 M Al₂(SO₄)₃ has a higher freezing point than 0.1 M of K₃[Fe(CN)₆].

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