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The normality of 10% (weight/volume) acetic acid is-
(A) 1N
(B) 10N
(C) 1.67N
(D) 0.83N

Last updated date: 23rd May 2024
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Hint: One of the expressions used to measure the concentration of a solution is 'Normality' in chemistry. It is abbreviated as 'N' and is often referred to as the corresponding solution concentration. It is vastly used in a solution and during titration reactions or especially when the acid-based chemistry is used as a measure of reactive species.

Complete step by step answer:
Since we know that the 10% (weight/volume) acetic acid as per given in the question means 10g acetic acid is added in 100ml of water.
Thus, from this information we can simply say that 100g of Acetic acid will be present in 1000ml of water.
As we already know that 60g has 1 mole of acetic acid.
Therefore, 100g will have-
$ \Rightarrow 100g = \dfrac{{100}}{{60}}$
$ \Rightarrow 1.67$ moles of $C{H_3}C{O_2}H$
Thus, we can see that 1.67 moles will be present in 1L of water.
This means that the solution is 1.67 moles.
Acetic acid has a chemical formula of $C{H_3}C{O_2}H$. In the case of acetic acid, 1N solution is equal to 1M solution.
Hence, the normality of 10% acetic acid as per calculated will be 1.67N.
Therefore, it is clear that option C is the correct option.

Note: The most powerful carboxylic acid, also known as ethanoic acid is the acetic acid $\left( {C{H_3}COOH} \right)$. A dilute (about 5% by volume) solution of acetic acid formed by fermentation and oxidation of natural carbohydrates is called vinegar. A salt, ester or acylal made of acetic acid is known as an acetate.