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The molal elevtion constant of water is ${{0.52}^{o}}C$. The boiling point of 1.0 molal aqueous KCl solution (asuming complete dissociation of KCl), therefore should be
Elevation in boiling point was ${{0.52}^{o}}C$ when $6gm$ of a compound $X$ was dissolved in $100gm$ of water. Molecular weight of $X$ is (${{K}_{b}}$ for water is 0.52 per $1000\ gm$ of water)
Increase in boiling point of a sucrose solution is 0.1 K, then what is increase in boiling point of the same concentration of NaCl solution
The boiling point of water $({{100}^{o}}C)$ becomes ${{100.52}^{o}}C$. If 3 grams of a nonvolatile solute is dissolved in $200\ ml$ of water. The molecular weight of solute is (${{K}_{b}}$ for water is $0.6\ K-m$)
The boiling point of a solution of 0.11 gm of a substance in 15 gm of ether was found to be 0.1°C higher than that of the pure ether. The molecular weight of the substance will be $\left[ {{K}_{b}}=2.16 \right]$
The latent heat of vaporisation of water is 9700 cal/mole and if the b.p. is ${{100}^{o}}C$, ebullioscopic constant of water is
The boiling point of a solution of $0.1050\ gm$ of a substance in 15.84 gram of ether was found to be ${{0.100}^{o}}C$ higher than that of pure ether. What is the molecular weight of the substance [Molecular elevaion constant of ether per 100 $g=21.6$]
Boiling point of chloroform was raised by 0.323 K, when 0.5143 g of anthracene was dissolved in its 35g. Molecular mass of anthracene is $({{K}_{b}}\text{for }CHC{{l}_{3}}=3.9\,k-kg\,mo{{l}^{-1}})$
When 10 g of a non-volatile solute is dissolved in 100 g of benzene, it raises boiling point by 1°C then molecular mass of the solute is $({{K}_{b}}\text{ for benzene }=\text{2}\text{.53 }k-{{m}^{-1}})$
0.15 gm of a substance dissolved in 15 g of solvent, boiled at a temperature higher by 0.216°C than that of the pure solvent. Find out the molecular weight of the substance (Molal elevation constant for the solvent is 2.16°C)

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