# Recent questions and answers in Solutions

### A solution containing $0.5\;g$ of a solute (molar mass 130 g\;mol^{-1})$in$50 \;g\;CCl_4$yields a boiling point elevation of boiling point . The molar mass of solute is about ### The solvent$CS_2$has enthalpy of vapourization of$352\;J\;g^{-1}$and boiling point equal to$320\;K$. The value of$K_b$for this solvent is about. ### A solvent of molar mass$84.2 \;g\;mol^{-1}$and boiling point$81.4^{\circ}C$has boiling point elevation constant equal to$ 2.79 \;K\;kg\;mol^{-1}$. Its molar enthalpy of vapourization will be about ### A sucrose solution in 50 g water boils at$100.15^{\circ}C$, If this solution is heated till its temperature is$100.375^{\circ}C$, how much of water is evaporated ? Given :$ K_b(water)=0.52\;K\;kg\;mol^{-1}$### An involatile solute A dimerizes in a solvent as$2A \rightleftharpoons A_2$. If m is the molarity of solute in the solution , then the equilibrium constant of the reaction is given as ### The elevation in boiling point when$20.16\;g$of freshly prepared$CuCl_2$(relative molar mass :$134.4$) is dissolved in$1\;kg$of water$(K_b=0.52\;kg\;K \;mol^{-1})$is ### When mercuric iodide is added to an aqueous solution of potassium iodide, the ### The elevation of boiling point of water produced by dissolving$1.17 g$sodium chloride in$100 g$water$K_b=0.512\;K\;kg\;mol^{-1})$is ### The boiling point of water at$735$Torr is$99.07^{\circ}C$. The mass of$NaCl$added in$100\;g$water$(K_b=0.51\;K\;kg\;mol^{-1})$to make its boiling point$100^{\circ}C$is ### For an ideal solution containing a nonvolatile solute, Which of the following expression is correctly represented ? ### Which of the following solvents has the largest value of$K_f$? ### The molar mass and the freezing point of camphor are$152.2\;g\;mol^{-1} $and$178.4^{\circ} C $respectively . The cryoscopic constant of camphor is$ 37.7\;K\;kg\;mol^{-1}$, the molar enthalpy of fusion of camphor is about ### If the freezing point depression constant of a solvent is$20.0\;K\;kg\;mol^{-1}$. If its$\Delta_{fus} H^0_m=2.74\;kJ\;mol^{-1}$and its molar mass is$84.2\;g\;mol^{-1}\$ the normal freezing point of the solvent would be about

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