The freezing point depression of `0.001 m K_(x)` `[Fe(CN)_(6)]` is `7.10xx10^(-3) K`. Determine the value of x. Given, `K_(f)=1.86 K kg "mol"^(-1)` for water.

The freezing point depression of 0.001mK_(x)[Fe(CN)_(6)] is 7.10xx10^(-3)K .Determine the value of x .Given , K_(f)=1.86 Kkg mol^(-1) for water

The freezing point depression of a 1.00 xx 10^-3 m solution of K_x[Fe(CN)_6] is 7.10xx10^-3 K. Determine x given K_f=1.86 K kg mol^-1 for H_2O . Assume 100% dissociation. K_f=1.86 Kkg mol ^-1 for H_2O

Freezing point depression of millimolal K_nFe(CN)_(6) is 7.1 xx 10^(-3) K. If K_f = 1.86 k Kg mol^(-1) . Calculate the value of n.

Freezing point depression of millimolal K_nFe(CN)_(6) is 7.1 xx 10^(-3) K. If K_f = 1.86 k Kg mol^(-1) . Calculate the value of n.

The freezing point (in .^(@)C) of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] (Mol.wt. 329) in 100 g of water (K_(f) = 1.86 K kg mol^(-1)) is

The freezing point (in .^(@)C) of a solution containing 0.1g of K_(3)[Fe(CN)_(6)] (Mol. wt. 329 ) in 100 g of water (K_(f) = 1.86 K kg mol^(-1)) is :

The freezing point (in .^(@)C) of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] (Mol.wt. 329) in 100 g of water (K_(f) = 1.86 K kg mol^(-1)) is

The freezing point (.^(@)C) of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] (molecular weight 329) on 100 g of water (K_(f)=1.86 K kg mol^(-1))