How is molar mass related to the elevation in boiling point of a solution ?
Discuss the depression of freezing point of a solution.
What is depression of freezing point ?
Write the equation relating depression in freezing point of a solution and the molar mass of the solute. Explain the terms.
Mole fraction of solute in some solution is 1//n . If 50% of solute molecules dissociate into two parts and remaining 50% get dimerised , new mole fraction of solvent becomes 4//5 . Find value of n.29. 0.1 M KI and 0.2 M are mixed in 3:1 volume ratio . The depression in freezing point of the resulting solution will be 0.1 x (Assume K_(f) of and molality =molarity). Then x=_________
Calculate the depression in the freezing point of a solution containing 0.1 g of K_(3)[Fe(CN)_(6)] in 100 g of H_(2)O ? (molecular weigth of K_(3)[Fe(CN)_(6)]=329, K_(f)=1.86K " kg mol"^(-1) )
Equal volumes of 1.0M AgNO_(3) and 1.0M KCl are mixed . The depression of freezing point of the resulting solution will be (K_(f)(H_(2)O)=1.86 K kg "mol"^(-1), 1M=1m)
19.5g of CH_(2)FCOOH is dissolved in 500g of water. The depression in freezing point of water observed is 1.0^(@)C . Calculate the Van't Hoff factor and dissociation constant of fluoroacetic acid.
45 g of ethylene glycol (C_(2)H_(6)O_(2)) is mixed with 600 g of water. Calculate (a) the freezing point depression and (b) the freezing point of the solution.
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
