(A) Given: $n_{\text{water}} = 1 \ mole$,$n_{\text{ethanol}} = 4 \ mole$. Total moles $= 1 + 4 = 5 \ moles$. Mole fraction of water $(X_{\text{water}}

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(A) Given: $n_{\text{water}} = 1 \ mole$,$n_{\text{ethanol}} = 4 \ mole$. Total moles $= 1 + 4 = 5 \ moles$. Mole fraction of water $(X_{\text{water}}) = \frac{n_{\text{water}}}{n_{\text{total}}} = \frac{1}{5} = 0.2$. Mole fraction of ethanol $(X_{\text{ethanol}}) = \frac{n_{\text{ethanol}}}{n_{\text{total}}} = \frac{4}{5} = 0.8$. Thus,the mole fraction of water is $0.2$ and ethanol is $0.8$.

Class 12 Chemistry Solutions Method of expressing concentration of solution

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$A$ solution contains $1 \ mole$ of water and $4 \ mole$ of ethanol. The mole fraction of water and ethanol will be

A
$0.2$ water + $0.8$ ethanol
B
$0.4$ water + $0.6$ ethanol
C
$0.6$ water + $0.8$ ethanol
D
$0.8$ water + $0.2$ ethanol

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Method of expressing concentration of solution

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The mole fraction of water in a $20\%$ aqueous solution of $H_2O_2$ is:

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$A$ solution contains $1 \ mole$ of water and $4 \ mole$ of ethanol. The mole fraction of water and ethanol will be

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$A$ solution is prepared by adding $2 \ g$ of $X$ to $1 \ mole$ of water. Mass percent of $X$ in the solution is $............. \ \%$

If $5.85 \ g$ of $NaCl$ (molecular weight $58.5$) is dissolved in water and the solution is made up to $0.5 \ L$,the molarity of the solution will be (in $M$)

The mass $\%$ of urea solution is $6$. The total weight of the solution is $1000 \ g$. What is its concentration in $mol \ L^{-1}$? (Density of water $= 1.0 \ g \ mL^{-1}$)$(C = 12 \ u, N = 14 \ u, O = 16 \ u, H = 1 \ u)$

An aqueous $KCl$ solution of density $1.20 \ g \ mL^{-1}$ has a molality of $3.30 \ mol \ kg^{-1}$. The molarity of the solution in $mol \ L^{-1}$ is ..... . (Nearest integer)[Molar mass of $KCl = 74.5 \ g \ mol^{-1}$]

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The mass $\%$ of urea solution is $6$. The total weight of the solution is $1000 \ g$. What is its concentration in $mol \ L^{-1}$? (Density of water $= 1.0 \ g \ mL^{-1}$)
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An aqueous $KCl$ solution of density $1.20 \ g \ mL^{-1}$ has a molality of $3.30 \ mol \ kg^{-1}$. The molarity of the solution in $mol \ L^{-1}$ is ..... . (Nearest integer)
[Molar mass of $KCl = 74.5 \ g \ mol^{-1}$]