0.4Molal solution of a complex compound in water has boiling point elevation in 0.4104 .Assume 50% dissociation.The formula of complex compound can be `K_(b)`= 0.52 for water

A solution containg 12 g of a non-electrolyte substance in 52 g of water gave boiling point elevation of 0.40 K . Calculate the molar mass of the substance. (K_(b) for water = 0.52 K kg mol^(-1))

The 0.0001 molal solution of a complex AB_(10) has the freezing point of -0.0015^(@)C in water. Assuming 100% dissociation of the complex, find the proper representation of the complex [K_(f)(H_(2)O=1.86Km^(-1))] (a) [AB_(8)] (b) [AB_(3)]B_(7) (c ) [AB_(7)]B_(3) (d) [AB_(5)]B_(5) .

The osmotic pressure of a dilute solution of an compound XY in water is four times that of a solution of 0.01 M BaCl_(2) in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY in solution is x xx 10^(–2) mol/L. The numerical value of x is____.

The osmotic pressure of a dilute solution of a compound XY in water is four times that of a solution of 0.01 M BaCl_(2) in water. Assuming complete dissociation of the given ionic compounds in water, the concentration of XY (in "mol" L^(-1) ) in solution is:

A solution containing 12.5g of a non electrolyte substance in 175g of water gave a boiling point elevation of 0.70 K. Calculate the molar mass of the substance. (Elevation constant for water, K_(b) = 0.52 K kg "mol"^(-1) )

A solution containing 12.5 g of non-electrolyte substance in 185 g of water shows boiling point elevation of 0.80 K. Calculate the molar mass of the substance. ( K_b=0.52 K kg mol^(-1) )

An octahedral complex is prepared by mixing CoCl3 and NH3 in the molar ratio 1 : 4, 0.1 m solution of this complex was found to freeze at 0.372°C. What is the formula of the complex? Given that molal depression constant (Kf) for water = 1.86°C/m.

A 0.001 molal aqueous solution of a complex [MA_8] has the freezing point of -0.0054^(@)C . If the primary valency of the salt undergoes 100% ionization and K_f for water =1.8 K molality^(-1) the correct representation of complex is

A solution of a non-volatile solute in water has a boiling point of 375.3 K. The vapour pressure of water above this solution at 338 K is: [Given p^(0) (water) = 0.2467 atm at 338 K and K_(b) for wate = 0.52 K kg mol^(-1) ]

A solution of urea in water has boiling point of 100.15^(@)C . Calculate the freezing point of the same solution if K_(f) and K_(b) for water are 1.87 K kg mol^(-1) and 0.52 K kg mol^(-1) , respectively.