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Question

What will be the molarity of a solution which contains $$5.85\; g$$ of $$NaCl(s)$$ per $$500$$ ml?


A
4molL1
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B
20molL1
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C
0.2molL1
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D
2molL1
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Solution

The correct option is C $$\displaystyle 0.2\: mol \:L^{-1}$$
The expression for the molarity of the solution is:

 $$Molarity  = \dfrac {\text {Mass of NaCl}}{\text {Molar mass of NaCl} \times \text {Volume of NaCl solution} (in\; L)}$$

Substituting values in the above expression, we get-

$$Molarity  = \dfrac {5.85} {58.5 \times 0.5} = \displaystyle 0.2\: mol \:L^{-1}$$

Hence, option C is correct.

Chemistry

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