$A$ solution of a nonvolatile solute is obtained by dissolving $3.5 \ g$ of solute in $100 \ g$ of solvent. The boiling point elevation is $0.35 \ K$. Calculate the molar mass of the solute. $(K_b = 2.5 \ K \ kg \ mol^{-1})$
- A$270 \ g \ mol^{-1}$
- B$260 \ g \ mol^{-1}$
- C$250 \ g \ mol^{-1}$
- D$240 \ g \ mol^{-1}$
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View Solution$A$ solution is prepared by dissolving a $2.5 \ g$ sample of an unknown compound in $34 \ g$ of benzene,$C_6H_6$. The solution boils at $1.38 \ ^\circ C$ higher than pure benzene. Which expression gives the molar mass of the unknown compound? $K_b$ of $C_6H_6$ is $2.53 \ ^\circ C \ m^{-1}$.
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View SolutionWhen $3.00 \, g$ of a substance $'X'$ is dissolved in $100 \, g$ of $CCl_4$,it raises the boiling point by $0.60 \, K$. The molar mass of the substance $'X'$ is $..... \, g \, mol^{-1}$. (Nearest integer).
$[$ Given $K_b$ for $CCl_4$ is $5.0 \, K \, kg \, mol^{-1} ]$
$[$ Given $K_b$ for $CCl_4$ is $5.0 \, K \, kg \, mol^{-1} ]$
An aqueous dilute solution containing non-volatile solute boils at $100.52^{\circ} C$. What is the molality of the solution (in $m$)? ($K_b = 0.52 \ K \ kg \ mol^{-1}$,boiling temperature of water $= 100^{\circ} C$)
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