The strength of a $10^{- 2} M N a_{2} C O_{3}$ solution in terms of its molality will be: $(density of solution = 1.10 {g mL}^{- 1}$ , $molecular weight of N a_{2} C O_{3} = 106 {g mol}^{- 1})$

9.00 \times 10^{- 3}

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1.50 \times 10^{- 2}

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5.10 \times 10^{- 3}

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11.2 \times 10^{- 3}

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Solution

The correct option is A $9.00 \times 10^{- 3}$
Given density of the solution $= 1.10 {g m L}^{- 1}$
Again, $10^{- 2} M N a_{2} C O_{3} = 10^{- 2} m o l N a_{2} C O_{3} in 1000 ml solvent$

$Mass of 1000 ml of the solution = (1.10 \times 1000) g = 1100 g$
$Mass of solvent = (1100 - 10^{- 2} \times 106 = 1098.94 g$
$∴ M o l a l i t y = \frac{10^{- 2}}{1098.94} \times 1000 \approx 9.00 \times 10^{- 3}$

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(density of solution = 1.10 {g mL}^{- 1}

molecular weight of N a_{2} C O_{3} = 106 {g mol}^{- 1})

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The strength of a 10−2 M Na2CO3 solution in terms of its molality will be: (density of solution=1.10 g mL−1,molecular weight of Na2CO3=106 g mol−1)

The correct option is A 9.00×10−3Given density of the solution =1.10 gmL−1 Again, 10−2 M Na2CO3=10−2 mol Na2CO3 in 1000 ml solvent Mass of 1000 ml of the solution=(1.10×1000) g=1100 g Mass of solvent=(1100−10−2×106=1098.94 g ∴ Molality=10−21098.94×1000≈9.00×10−3

The strength of a $10^{- 2} M N a_{2} C O_{3}$ solution in terms of its molality will be: $(density of solution = 1.10 {g mL}^{- 1}$ , $molecular weight of N a_{2} C O_{3} = 106 {g mol}^{- 1})$