Calculate depression of freezing point for 0.56 molal aq. Solution of KCl. (Given : K_f(H_(2)O) = 1.8 kg mol^(-1) ).
If 30 g a solute of molecular mass 154 is dissolved in 250 g of benzene. What will be the elevation in boiling point of the resuling solution ? (Given : K_B(C_(6)H_(6)) =2.6 K kg mol^(-1) )
Calculate the boiling point of a one molar aqueous solution of KBr (density 1.06g mL^-1) . ( K_b for water= 0.52kgmol^-1 , atomic masses: K=39, Br=80)
Calculate the boiling point of one molar aquesous solution (density 1.03gmL^-1) of NaCl. K_b for water= 0.52Km^-1 .
An aqueous solution of 0.01 M KCl cause the same elevation in boiling point as an aqueous solution of urea. The concetration of urea solution is : a) 0.01 m b) 0.005 M c) 0.02 M d) 0.04 M
0.1 M KI and 0.2 M AgNO_(3) are mixed in 3 : 1 volume ratio. The depression of freezing point of the resulting solution will be [ K_(b)(H_(2)O) = 1.86 K kg "mol"^(-1) ]:
Calculate the freezing point of a one molar aqueous solutoin (density 1.04gL^-1) of KCl. ( K_f of water=1.86Kg mol^-1 , atomic masses of K=39, Cl=35.5)
The elevation of boiling point for 1M urea, 1M glucose, 1M NaCl and 1M K_2SO_4 are in the ratio
If the elevation in boiling point of a solution of 10 gm of solute (mol. Wt. = 100) in 100 gm of water is DeltaT_(b) , the ebullioscopic constant of water is
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
