An aqueous solution containing 12.48g of barium chloride in 1.0kg of water boils at 373.0832K. Calculate the degree of dissociation of barium chloride. (Given Kb for water= 0.52K/m) Share with your friends Share 17 Geetha answered this According to elevation of boiling point,∆Tb = Kb × m = Kb × W2M2 × W1 ∆Tb - elevation of boiling pointKb - molal elevation constantW2 - Weight of the soluteM2 - Molecular mass of the soluteW1 - Weight of the solvent∆Tb = Kb × W2M2 × W1 × 1000 = 0.52 × 12.48208.23× 1 = 0.0312∆Tb (given) = Tb - Tb0 = 373.0832 - 373 = 0.0832Degree of dissociationα = i-1n -1Where i = Vant Hoff factori = Observed colligative propertyCalculated colligative property = 0.08320.0312 = 2.67α = 2.67-13 -1 (where n = 3 as BaCl2 dissociates BaCl2 → Ba2+ + 2Cl- = 1.672 = 0.8333 = 0.8333 × 100 = 83.33 % 44 View Full Answer