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Standard XII

Chemistry

Depression in Freezing Point

The cryoscopi...

Question

The cryoscopic constant of water is 1.86 K kg $m o l^{- 1}$ . A 0.01 molal acetic acid solution produces a depression of ${0.0194}^{0} C$ in the freezing point. The degree of dissociation of acetic acid is:

zero

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0.043

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0.43

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Solution

The correct option is A 0.043
Given $K_{1} = 1.86 K$ kg $m o l^{- 1}$ , $m = 0.01$
$Δ T_{f} = {0.0194}^{\circ} C$
$∴ Δ T_{f} = i . K_{f} m; \frac{0.0194}{1.86 \times 0.01} = i$
or $i = 1.043$ or $α = 0.043$

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The cryoscopic constant of water is 1.86 K kg mol−1. A 0.01 molal acetic acid solution produces a depression of 0.01940C in the freezing point. The degree of dissociation of acetic acid is:

The correct option is A 0.043Given K1=1.86K kg mol−1, m=0.01ΔTf=0.0194∘C∴ΔTf=i.Kfm;0.01941.86×0.01=ior i=1.043 or α=0.043

The cryoscopic constant of water is 1.86 K kg $m o l^{- 1}$ . A 0.01 molal acetic acid solution produces a depression of ${0.0194}^{0} C$ in the freezing point. The degree of dissociation of acetic acid is:

The correct option is A 0.043
Given $K_{1} = 1.86 K$ kg $m o l^{- 1}$ , $m = 0.01$
$Δ T_{f} = {0.0194}^{\circ} C$
$∴ Δ T_{f} = i . K_{f} m; \frac{0.0194}{1.86 \times 0.01} = i$
or $i = 1.043$ or $α = 0.043$