The density of a $10.0 \% \, w/w$ aqueous solution of $KCl$ is $1.06 \, g \, cm^{-3}$. The molarity of this solution is .........
- A$1.489 \, M$
- B$1.420 \, M$
- C$1.489 \, mol/kg$
- D$1.420 \, mol/kg$
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Dissolving $120 \ g$ of a compound (mol. wt $= 60$) in $1000 \ g$ of water gave a solution of density $1.12 \ g \ mL^{-1}$. The molarity of the solution is: (in $M$)
Molality of $0.8 \ M \ H_2SO_4$ solution (density $1.06 \ g \ cm^{-3}$) is . . . . . . $\times 10^{-3} \ m$.
If the mole fraction of the solute in benzene is $0.2$,then the molality of the solution is .........
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View SolutionWhat is mole fraction? Explain in brief.
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