The freezing point of `1` molal `NaCl` solution assuming `NaCl` to be `100%` dissociated in water is:

The freezing point of 1 molar NaCl solution assuming NaCl to be 100% dissociated in water is: ( K_f = 1.86 K molality^-1 )

The freezing point of one molal NaCl solution assuming NaCl to be 100% dissociated in water is (molal depression constant= 1.86)

The freezing point of one molal NaCl solution assuming NaCI to be 100% dissociated in water is (molal depression constant is 1.86)

Calculate the freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water. ( K_(f) for water = 1.86^(@)"mol"^(-) ).

Fill in the blanks choosing appropriate word/words from these given in the brackets : (increases, decreases, the highest, the lowest, elevation, directly depression, molality, mole fraction, gt 1, lt 1, DeltaV, DeltaS , number of solute particles, nature of solute particles, hypotonic, T, - 3.72^(@)C, -1.86^(@)C , zero, one, two, more than, less than, 1 kg, 1 mole, molal, same extent, solution, equivalent.) The freezing point of 1 m NaCl solution assuming NaCl to be 100% ionized in water is......

The molality of 2% (W/W) NaCl solution nearly