Question

6g of NaOH are dissolved in 200 cm3 of water. What is the relation between molarity

and normality of the solution thus obtained ?​

Answer 1

very easy one ........well hope it helps ^^

Answer 2

The relation between molarity and normality of the solution thus obtained are equal.

Explanation:

Molarity is defined as the number of moles dissolved per liter of the solution.

$Molarity=\frac{moles\times 1000}{\text {volume in ml}}$

moles of $NaOH=\frac{\text {given mass}}{\text {Molar mass}}=\frac{6g}{40g/mol}=0.15$

$Molarity=\frac{0.15\times 1000}{200ml}=0.75M$

Normailty is defined as number of gram equivalents present per litre of the solution.

$Normality=\frac{\text {gram equivalents\times 1000}}{\text {volume in ml}}$

Equivaent mass =$\frac{\text {Molar mass}}{acidity}=\frac{40}{1}=40$

gram equivalents of $NaOH=\frac{\text {given mass}}{\text {equivalent mass}}=\frac{6g}{40g/mol}=0.15$

$Normality=\frac{0.15\times 1000}{200ml}=0.75N$

Thus relation between molarity and normality of the solution thus obtained are equal.

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