The freezing point of 1 m NaCl solution ...

The freezing point of `1 m NaCl` solution assuming `NaCl` to be `100%` dissociated In water is `(K_(f)=1.86 K m^(-1))`

`-1.86^(@)C`

`-3.72^(@)C`

`+1.86^(@)C`

`+3.72?^(@)C`

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

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 freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

The lowering in freezing point of 0.75 molal aqueous solution NaCI (80% dissociated) is [Given, K_f, for water 1.86 K kg mol^(-1)]

What will be the freezing point of a 0.5 m KCl solution ? The molal freezing point constant of water is 1.86^@C m^(-1) .

What would be the freezing point of aqueous solution containing 17 g of C_(2)H_(5)OH in 100 g of water (K_(f) H_(2)O = 1.86 K mol^(-1)kg) :

The freezing point of a solution that contains 10 g urea in 100 g water is ( K_1 for H_2O = 1.86°C m ^(-1) )

A weak electrolyte XY is 5% dissociated in water. What is the freezing point of a 0.01 molal aqueous solution of XY ? The cryoscopic constant of water is 1.86 K/m.

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