If sodium sulphate is considered to be completely dissociated into cations

Question:

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water $\left(\Delta \mathrm{T}_{\mathrm{f}}\right)$, when $0.01 \mathrm{~mol}$ of sodium sulphate isdissolved in $1 \mathrm{~kg}$ of water, is $\left(\mathrm{K}_{\mathrm{f}}=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}\right)$ :-

 

  1. 0.0186 K

  2. 0.0372 K

  3.  0.0558 K

  4. 0.0744 K


Correct Option: , 3

Solution:

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