Which of the following aqueous solutions cont | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The boiling point elevation is a colligative property,which depends on the number of particles in the solution. The formula for boiling point elev

Vedclass · Accepted Answer

$NaCl$ solution

Vedclass · Answer

(A) The boiling point elevation is a colligative property,which depends on the number of particles in the solution. The formula for boiling point elevation is $\Delta T_b = i 	imes K_b 	imes m$. Since the mass of the solute is the same $(10 \ g)$,the molality $(m)$ is inversely proportional to the molar mass $(M)$ of the solute. $NaCl$ $(M \approx 58.5 \ g/mol)$ and $KCl$ $(M \approx 74.5 \ g/mol)$ are electrolytes with a van't Hoff factor $(i)$ of $2$,while sugar ($C_{12}H_{22}O_{11}$,$M \approx 342 \ g/mol$) and glucose ($C_6H_{12}O_6$,$M \approx 180 \ g/mol$) are non-electrolytes $(i = 1)$. Comparing $NaCl$ and $KCl$,$NaCl$ has a lower molar mass,resulting in a higher molality $(m)$. Therefore,$NaCl$ produces the highest number of particles per unit mass,leading to the highest boiling point.

Which of the following aqueous solutions containing $10 \ g$ of solute in each case has the highest boiling point $(B.P.)$?

Similar Questions

The molal elevation constant of water is $0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar is dissolved in $200 \ g$ of water,at what temperature $(^oC)$ will the solution start to boil under $1 \ bar$ pressure?

The boiling point of $0.2 \, mol \, kg^{-1}$ solution of $X$ in water is greater than equimolal solution of $Y$ in water. Which one of the following statements is true in this case?

$A$ solution containing $2 \ g$ of a non-volatile solute in $20 \ g$ of water boils at $373.52 \ K$. The molecular mass of the solute is $....... \ g \ mol^{-1}$. (Nearest integer) Given,water boils at $373 \ K$,$K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$.

If the boiling point of a urea solution is $100.18^{\circ}C$ and $K_b$ for water is $0.512 \ K \ kg \ mol^{-1}$,what is the molality of the solution? (Boiling point of water $= 100^{\circ}C$)

Calculate the amount of solute dissolved in $160 \ g$ of solvent that boils at $85^{\circ}C$. The molar mass of the solute is $120 \ g \ mol^{-1}$. $(K_{b}$ for solvent $= 2.7^{\circ}C \ kg \ mol^{-1}$ and boiling point of pure solvent $= 76^{\circ}C)$ (in $g$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module