0.1 molal solution of `Hg(NO_(3))_(2)` freezes at `-.558^(@)` C. The cryoscopic constant for water is 1.86 KKg `mol^(-1)` then what will be the percentage ionisation of salt ?

0.1 molal solution of Hg(NO_(3))_(2) freezes at 0.558^(@) C. The cryoscopic constant for water is 1.86 KKg mol^(-1) then what will be the percentage ionisation of salt ?

The freezing point of 0.1 molal aq. Solution of K_(X)[Fe(CN)_(6)] is -0.744^(@) C. The molal depression constant of water is 1.86 K-kg mol^(-1) . If the salt behaves as strong electrolyte in water, the value of X is :

The freezing point of a 1.00 m aqueous solution of HF is found to be -1.91^(@)C . The freezing point constant of water, K_(f) , is 1.86 K kg mol^(-1) . The percentage dissociation of HF at this concentration is:-

The freezing point of a 1.00 m aqueous solution of HF is found to be -1.91^(@)C . The freezing point constant of water, K_(f) , is 1.86 K kg mol^(-1) . The percentage dissociation of HF at this concentration is:-

The freezing point of a 1.00 m aqueous solution of HF is found to be -1.91^(@)C . The freezing point constant of water, K_(f) , is 1.86 K kg mol^(-1) . The percentage dissociation of HF at this concentration is:-

The molal freezing point constant for water is 1.86 K . Kg "mole"^(-1) . The freezing point of 0.1 m NaCl solution is