Question

Calculate the Normality of 9.8% w/v of sulphuric acid

Answer 1

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Answer 2

The Normality of 9.8% w/v of sulphuric acid is$1.4 N$

Explanation:

• 9.8% w/v of the sulphuric acid  $H2SO4$ solution means  $9.8 gm$ of solute dissolved in $100 g$ of solution.
• Density of the sulphuric acid  $H2SO4$ solution means $=1.2 g/ml$
• Volume$=\frac{Mass}{density}$    It  is the amount of mass divided by the density of the substance.
• Volume =$\frac{100}{1.2}$
• Volume utilised is $83.33 ml$
• Molarity $= \frac{98*83.33}{9.8*1000}$
• ​$=1.2 M$
• Normality =Molarity × number of hydrogen ions
• Normality = $1.2$×$2=1.4 N$
• Normality is defined as the number of gram equivalent dissolved in one liter of solution.
• Molarity is defined as number of moles of the solute dissolved in one liter of the solution.