The molal elevation constant of water is 0.51. The boiling point of 0.1 molal aqueous NaCl solution is nearly :

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K m^(-1) . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl ) should be

The molal elevation constant of water = 0.52 K, molality^-1 . The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl), should be:

Calculate the molal elevation constant , "K"_("b") for water and the boiling point of 0.1 molal urea solution. Latent heat of vaporisation of water is 9.72 kcal "mol"^(-1) at 373.15K.

Calculate the molal elevation constant of water , it being given that 0.1 molal aqueous solution of substance boiled at 100.052^@ C .