A solution containing 0.85 ~g of ZnCl ₂ in 125.0 ~g of water freezes at -0.23^ C . The apparent degree of dissociation of the salt is (K_f . for water =1.86 ~K ~kg ~mol ⁻¹ , atomic mass: Zn =65.3 and Cl =35.5)

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Correct answer: B. 73.5 %

Mol.wt. = k_f w 1000 T_f W = 1.86 0.85 1000 0.23 125 55 gm Where aligned & w=0.85 ~g & W=125 ~g & T_f=0^ C - (-23^ C )=23^ C aligned Now, i= M_ normal M_ observed = 136.3 55 =2.47 aligned & 1- ZnCl ₂ Zn ⁺⁺ + 2 2 Cl ⁻ & Van't Hoff factor ( i ) & = 1- + +2 1 =2.47 & =0.735=73.5 % & aligned

A solution containing 0.85 ~g of ZnCl ₂ in 125.0 ~g of water freezes at -0.23^ C . The apparent degree of dissociation of the salt is (K_f . for water =1.86 ~K ~kg ~mol ⁻¹ , atomic mass: Zn =65.3 and Cl =35.5)

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