Calculate the molecular weight of a substance whose `7.0%` (by weight) solution in water freezes at `-0.89^(@)C`. `(k_(f) "for" H_(2)O=1.86K"molality"^(-1)`).

Calulate the molesules mass of a substance whose 7.0% by mass solution in water freezes at -0.93^(@)C . the cryosctopic constant of water is 1.86^(@)C kg mol^(-1) :

Calulate the molesules mass of a substance whose 7.0% by mass solution in water freezes at -0.93^(@)C . the cryosctopic constant of water is 1.86^(@)C kg mol^(-1) :

6 grams of a substance 'A' dissolved in 100 g of water freezes at - 0.93^(@)C . The molecular mass of 'A' is ( K_(f)=1.86 Km^(-1) ).

The freezing point of 0.08 molal NaHSO_(4) is -0.345^(@)C . Calculate the percentage of HSO_(4)+O ions that transfers a proton to water. Assume 100% ionization of NaHSO_(4) and K_(t) for H_(2)O = 1.86 K molality^(-1) .

The freezing point of 0.08 molal NaHSO_(4) is -0.345^(@)C . Calculate the percentage of HSO_(4)+O ions that transfers a proton to water. Assume 100% ionization of NaHSO_(4) and K_(t) for H_(2)O = 1.86 K molality^(-1) .

The freezing point of 0.08 molal NaHSO_(4) is -0.345^(@)C . Calculate the percentage of HSO_(4)+O ions that transfers a proton to water. Assume 100% ionization of NaHSO_(4) and K_(t) for H_(2)O = 1.86 K molality^(-1) .

Calculate the molecular weight of a substance if the freezing point of a solution containing 100 g of benzene and 0.2 g of the substance is 0.17 K below that of benzene. The cryoscope constant of benzerne is 5.16 K kgmol^(-1)

0.1 mole of sugar is dissolved in 250 g of water. The freezing point of the solution is [K_(f) "for" H_(2)O = 1.86^(@)C "molal"^(-1)]