Calculate the boiling point of solution containing `0.456g` of camphor (molar mass =152 ) dissolved in `31.4g` of acetone (boiling point `=56.30^(@)C` ), if the molar elevation constant per 100g of acetone is `17.2^(@)C.`

Calcualte the boiling point of a solution containing 0.456g comphore (mol.mass = 152) dissolved in 31.4g of acetone (b.p 56.3^@C ), if the molecular elevation constant per 1000g of acetone is 17.2^@C

Calculate the biling point of a solution containing 0.456 g of comphor (molar mass=152 g mol^(-1)) dossoved in 31.4 g of acetone(b.p.= 329.45 K). Given that the molecular elevation constant per 100 g of solvent is 17.2 K.

Calculate the boiling point of a solution containing 0.45g of camphor (mol. wt. 152) dissolved in 35.4g of acetone (b.p 56.3^@C ), K_b per 100 gm of acetone is 17.2^@C

A solution contains 0.524 g of camphor ( molar mass = 152 g/ mol dissolved in 36.8 g of ether (boiling point =34.6^(@) C) . The molal elevation constant per 100 g of ether is 19.4 K kg mol ^(-1) . The boiling point of the solution is _______.

Calculate the molarity of a solution containing 2.8g of KOH per litre (molar mass of KOH = 56).

The boiling point of a glucose solution containing 12 g of glucose in 100 g of water is 100.34^@C . Boiling point of water is 100^@C . The molal elevation constant of water is

The boiling point of a glucose solution containing 12 g of glucose in 100 g of water is 100.34^@C . Boiling point of water is 100^@C . The molal elevation constant of water is