A 1 molal K4[Fe(CN)6] solution has a degree of dissociation of 0.4. Its boiling point is equal to that of another solution which contains 18.1 weight percent of a non electrolytic solute A. The molar mass of A is ______ u. (Round off to the nearest integer).
[Density of water = 1.0 g cm?³]
A 1 molal K4[Fe(CN)6] solution has a degree of dissociation of 0.4. Its boiling point is equal to that of another solution which contains 18.1 weight percent of a non electrolytic solute A. The molar mass of A is ______ u. (Round off to the nearest integer).
[Density of water = 1.0 g cm?³]
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1 Answer
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For the dissociation of K? [Fe (CN)? ]? 4K? + [Fe (CN)? ]? , the number of ions produced (n) is 5.
The degree of dissociation (α) is related to the van't Hoff factor (i) by α = (i-1)/ (n-1).
Given α = 0.4: 0.4 = (i - 1) / (5 - 1) => 1.6 = I - 1 => I = 2.6
Using the depression in freezing point formula (ΔTf = i·Kf·m), and equating the ΔTf for two different solutions:
ΔTf (K? [Fe (CN)? ]) = ΔTf (A)
i? ·Kf·m? = i? ·Kf·m?
(2.6) × [ (18.1 / M) / (100-18.1)/1000] = (1) × [ (w? /M? ) / (W? /1000)]
The problem simplifies to finding the molar mass M of s...more
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