To observe an elevation of boiling point of `0.05^(@)C`, the amount of a solute (molecular weight = 100) to be added to 100 g of water `(K_(b) = 0.5)` is

To observe an elevation of boiling point of 0.05^(@)C , the amount of a solute (molecular weight = 100) to be added to 100 g of water (K_(b) = 0.5^(@)Ckgmol^-1) is

To observe an elevation of boiling point at 0.05^@C , the amount of solute (mol.wt =100) to be added to 100g of water (k_b=0.5) is

If the elevation in boiling point of a solution of 10 g of solute (molecular weight = 100) in 100 g of water is Delta T_(b) , the ebullioscopic constant of water is

If the elevation in boiling point of a solution of 10 g of solute (molecular weight = 100) in 100 g of water is Delta T_(b) , the ebullioscopic constant of water is

2g of a non-electrolyte solute dissolved in 200 g of water shows an elevation of boiling point of 0.026^(@)C. K_(b) of water is 0.52 K . "mole"^(1) kg then the molecular weight of solute is x xx100 . What is the value of 'x'?

Elevation in boiling point was 0.52^(@)C when 6 g of a compound X was dissolved in 100 g of water. Molecular weight of X is ( K_(b) of water is 5.2^(@)C per 100 g of water)

Elevation in boiling point was 0.52^(@)C when 6 g of a compound X was dissolved in 100 g of water. Molecular weight of X is ( K_(b) of water is 5.2^(@)C per 100 g of water)