The normal freezing point of nitrobenzne...

The normal freezing point of nitrobenzne `(C_(6)H_(5)NO_(2))` is 278.82 K.A 0.25 m solution of solute A in nitrobenzene decreases the freezing point to 276.82 K. The value of `K_(f)` for nitrobenzene is

2K kg `mol^(-1)`

4K kg `mol^(-1)`

6K kg `mol^(-1)`

8.0K kg `mol^(-1)`

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The normal freezing point of nitrobenzene (C_(6)H_(5)NO_(2)) is 278.82K . A 0.25 molal solution of a certain solute in nitrobenzene causes a freezing point depression of 2 degrees. Calculate the value of K_(f) for nitrobenzene.

The freezing point of pure nirobenzene is 278.8 K. When 2.5 g of an unknown substance is dissoved in 100 g of introbenzene, the freezing point of the solution is found to be 276.8 K. If the freezing point depression of nitrobenzene is 8.0 K kg mol^(-01) , What is the molar of the unknow substance ?

The vapour pressure of pure benzene at 25^@C is 640.0 mm Hg and vapour pressure of a solution of a solute in benzene is 25^@C is 632.0 mm Hg. Find the freezing point of the solution if k_f for benzene is 5.12 K/m. (T_("benzene")^@ = 5.5^@C)

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A 0.025 m solution of monobasic acids has a freezing point of -0.060^(@)C . What are K_(a) and pK_(a) of the acid? (K_(f)=1.86^(@)C)

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