Calculate the molarity of $11.7 %$ by mass of $N a C l$ in water. The density of the solution is $1.60 g / m L$ .
(Given, atomic mass $N a = 23 u, C l = 35.5 u$ )

1.6 M

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4.2 M

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3.2 M

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2 M

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Solution

The correct option is C $3.2 M$
Asssuming $100 g$ of the solution,
Mass of $N a C l = 11.7 g$
Molar mass of $N a C l = 23 + 35.5 = 58.5 g$
$∴$ Moles of $N a C l = \frac{11.7}{58.5}$ = 0.2
Mass of the solution = 100 g
Volume of the solution $= \frac{Mass}{Density} = \frac{100}{1.6} = 62.5 m L$

$Molarity = \frac{moles}{volume (L)} = \frac{0.2}{0.0625} = 3.2 M$

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Similar questions

11.7 %

N a C l

1.60 g / m L

N a = 23 u, C l = 35.5 u

N a C l

[N a = 23 u, C l = 35.5 u]

{N a}^{+}

{C l}^{-}

N a C l

2.165 g {c m}^{- 3}

N a - 23 u, C l = 35.5 u

6.023 \times 10^{23}

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