What is the freezing point of a solution containing `8.1g Br `in `100g` water assuming the acid to be `90%`ionised(`K_(f)`for water =`1.8K "mole"^(-1))`

Calculate the freezing point of a solution containing 8.1 g of HBr in 100g of water, assuming the acid to be 90% ionized. [Given : Molar mass Br = 80 g/mol, K_(f) water = 1.86 K kg/mol].

Calculate the freezing point of a solution containing 8.1 g of HBr in 100g of water, assuming the acid to be 90% ionized. [Given : Molar mass Br = 80 g/mol, K_(f) water = 1.86 K kg/mol].

Ethylene glycol ("molar mass"=62 g mol^(-1)) is a common automobile antyfreeze. Calculate the freezing point of a solution containing 12.4 g of this substance in 100 g of water. (Given K_(f) for water = 1.86 K kg mol^(-1))

Calculate the freezing point of a solution containing 0.5 g KCl (Molar mass = 74.5 g/mol) dissolved in 100 g water, assuming KCl to be 92% ionized. K_(f) of water = 1.86 K kg/mol.

Calculate the freezing point of a solution containing 0.5 g KCl (Molar mass = 74.5 g/mol) dissolved in 100 g water, assuming KCl to be 92% ionized. K_(f) of water = 1.86 K kg/mol.

What should be the freezing point of aqueous solution containing 17g of C_(2)H(5)OH is 1000g of water ( K_(f) for water = 1.86 deg kg mol^(-1) )?

What should be the freezing point of aqueous solution containing 17g of C_(2)H_(5)OH in 1000g of water ( K_(f) for water = 1.86 deg kg mol^(-1)) ?