$4 L$ of $0.02 M$ aqueous solution of $N a C l$ was diluted by adding one litre of water. The molarity of the resultant solution is :

0.004

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0.008

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0.012

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0.016

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Solution

Correct option: (D)
Analyzing the given conditions:
$M_{1} = 0.02 M$
$V_{1} = 4 L$
After dilution, 1 L of water is added
$M_{2} = ?$
$V_{2} = (4 + 1) L = 5 L$
According to molarity equation
$M_{1} V_{1} = M_{2} V_{2}$
So, $0.02 \times 4 = M_{2} \times 5$
$M_{2} = 0.016 M$
Thus, the correct option is A.

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4L of 0.02M aqueous solution of NaCl was diluted by adding one litre of water. The molarity of the resultant solution is :

Correct option: (D)Analyzing the given conditions:M1=0.02MV1=4LAfter dilution, 1 L of water is addedM2=?V2=(4+1)L=5LAccording to molarity equationM1V1=M2V2So, 0.02×4=M2×5 M2=0.016MThus, the correct option is A.

$4 L$ of $0.02 M$ aqueous solution of $N a C l$ was diluted by adding one litre of water. The molarity of the resultant solution is :