Understanding the Normality of 0.1 Molar Oxalic Acid

In chemistry, understanding the concentration of solutions is crucial for various applications, from laboratory experiments to industrial processes. This article will delve into the specific question of the normality ((N)) of a 0.1 molar (M) solution of oxalic acid (H2C2O4).

What is Molarity (M)?

Molarity, often denoted as (M), is a measure of concentration of a solution. It is defined as the number of moles of solute dissolved in one liter of solution. This can be expressed mathematically as:

(M frac{text{moles of solute}}{text{liters of solution}})

What is Normality ((N))?

Normality ((N)) is a measure of concentration that takes into account the number of equivalents of the solute per liter of solution. One equivalent (or gram equivalent) is the quantity of a substance that will convert one mole of hydrogen ion (H(^ )) or hydroxide ion (OH(^-)) in a reaction. The formula to calculate normality in term of mole is:

(N M times n)

where (n) is the number of equivalents of the solute per mole.

Molecular Weight and Equivalent Weight of Oxalic Acid

Oxalic acid (H2C2O4) has a molecular weight of 90 g/mol. It can act as a diprotic acid, meaning it can donate two protons (H ) per molecule in a reaction, like this:

H2C2O4 2H → 2H2O C2O42-

Therefore, the equivalent weight of oxalic acid is 45 g/eq, which is half of its molecular weight.

1 Molar Oxalic Acid and its Normality

A 1 molar (1 M) solution of oxalic acid contains 1 mole of oxalic acid per liter of solution. Given that oxalic acid can donate two protons per molecule, it has a normality of 2 equivalents per liter (2 N).

The relationship between molarity ((M)) and normality ((N)) for oxalic acid can be expressed as:

(N 2M)

Therefore, the 0.1 molar (0.1 M) solution of oxalic acid will have a normality of:

(N 2 times 0.1 0.2 N)

Applications and Importance in Chemistry

Understanding the normality of oxalic acid solutions is important in various chemical reactions and applications. For example, in titrations, normality is often used instead of molarity because it directly relates to the number of titrant equivalents required to neutralize a given amount of analyte.

Conclusion

Understanding the relationship between molarity and normality in oxalic acid solutions is fundamental for accurate chemical calculations and ensuring the proper functioning of experimental procedures. Whether in educational settings or industrial applications, knowing these concentrations ensures precise and reliable results.