Chemistry, asked by khushal546, 9 months ago

What is normality of 1.2M CH3COOH solution

Answers

Answered by Phaneendhar

Answer:

1.2

Explanation:

Normality=Molarity×n-factor

N=M×n

n for CH3COOH is 1

So, N=1.2×1=1.2

Answered by abhi12shakya

Answer: The normality of a 1.2 M solution of acetic acid is 1.2 N.

Explaination:

For acetic acid (CH3COOH), the equivalent weight is equal to its molecular weight divided by the number of acidic hydrogen atoms it has. Acetic acid has one acidic hydrogen atom, so its equivalent weight is 60g/mol.

Now we find the normality by the formula,

Normality = Molarity x Number of Equivalents per Mole

Normality = 1.2 M x 1 equivalent/mole

Normality = 1.2 N.

Normality

Normality is a measure of the concentration of a solution and is defined as the number of gram-equivalents of solute per liter of solution

Normality is used in acid-base titrations to determine the unknown concentration of an acid or a base.

Molarity

Molarity is a unit of concentration that is commonly used in chemistry. It is defined as the number of moles of a solute present in one liter of solution.

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