An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7g of water freezes at 272.813 K. If the value of K_f for water is 1.86 K/m, what is the molecular mass of the monobasic acid?

50 g/mole

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46 g/mole

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55 g/mole

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60 g/mole

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Solution

The correct option is
D

60 g/mole
Given that,
Weight of solutem= 0.1g
Weight of solvent =21.7g
$K_{f}$ for water = 1.86 K/m
$Δ T_{f} = F r e e z i n g p o i n t o f w a t e r - F r e e z i n g p o i n t o f s o l u t i o n$
=273-272.813 = 0.337K
$m = \frac{1.86 \times 0.1 \times 1000}{0.037 \times 21.7} = \frac{60 g}{m o l}$

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An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7g of water freezes at 272.813 K. If the value of Kf for water is 1.86 K/m, what is the molecular mass of the monobasic acid?

The correct option is D 60 g/moleGiven that,Weight of solutem= 0.1gWeight of solvent =21.7gKffor water = 1.86 K/mΔTf=Freezingpointofwater−Freezingpointofsolution =273-272.813 = 0.337Km=1.86×0.1×10000.037×21.7=60gmol

An aqueous solution of a weak monobasic acid containing 0.1 g in 21.7g of water freezes at 272.813 K. If the value of K_f for water is 1.86 K/m, what is the molecular mass of the monobasic acid?