(B) Mass of urea $= 6\% \text{ of } 1000 \ g = \frac{6}{100} \times 1000 = 60 \ g$.$Molar \text{ mass of urea } (NH_2CONH_2) = 14 + 2 + 12 + 16 + 14 +

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(B) Mass of urea $= 6\% \text{ of } 1000 \ g = \frac{6}{100} \times 1000 = 60 \ g$.$Molar \text{ mass of urea } (NH_2CONH_2) = 14 + 2 + 12 + 16 + 14 + 2 = 60 \ g \ mol^{-1}$.Moles of urea $= \frac{60 \ g}{60 \ g \ mol^{-1}} = 1 \ mol$.Since the density of the solution is assumed to be $1.0 \ g \ mL^{-1}$,the volume of $1000 \ g$ solution $= 1000 \ mL = 1 \ L$.Molarity $= \frac{\text{Moles of solute}}{\text{Volume of solution in } L} = \frac{1 \ mol}{1 \ L} = 1.0 \ mol \ L^{-1}$.

Class 12 Chemistry Solutions Method of expressing concentration of solution

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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 $= 1.0 \ g \ mL^{-1}$)
$(C = 12 \ u, N = 14 \ u, O = 16 \ u, H = 1 \ u)$

AP EAMCET 2024 All AP EAMCET

A
$1.5$
B
$1.064$
C
$1.12$
D
$0.80$

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Method of expressing concentration of solution

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If the molality of an aqueous solution is $m$ and the mole fraction of the solute is $y$,which of the following relations is correct?

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Define the following terms:
$(i)$ Mole fraction $(ii)$ Molality $(iii)$ Molarity $(iv)$ Mass percentage

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When $100 \ mL$ of $2 \ M \ KCl$ and $200 \ mL$ of $3 \ M \ K_2SO_4$ solutions are mixed,what will be the molarity of $K^+$ ions in the resulting mixture (in $M$)?

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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 $M$)

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$x$ grams of water is mixed in $69 \ g$ of ethanol. The mole fraction of ethanol in the resultant solution is $0.6$. What is the value of $x$ in grams?

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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 $= 1.0 \ g \ mL^{-1}$)$(C = 12 \ u, N = 14 \ u, O = 16 \ u, H = 1 \ u)$

Similar Questions

If the molality of an aqueous solution is $m$ and the mole fraction of the solute is $y$,which of the following relations is correct?

Define the following terms:$(i)$ Mole fraction $(ii)$ Molality $(iii)$ Molarity $(iv)$ Mass percentage

When $100 \ mL$ of $2 \ M \ KCl$ and $200 \ mL$ of $3 \ M \ K_2SO_4$ solutions are mixed,what will be the molarity of $K^+$ ions in the resulting mixture (in $M$)?

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 $M$)

$x$ grams of water is mixed in $69 \ g$ of ethanol. The mole fraction of ethanol in the resultant solution is $0.6$. What is the value of $x$ in grams?

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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 $= 1.0 \ g \ mL^{-1}$)
$(C = 12 \ u, N = 14 \ u, O = 16 \ u, H = 1 \ u)$

Define the following terms:
$(i)$ Mole fraction $(ii)$ Molality $(iii)$ Molarity $(iv)$ Mass percentage