Preparation of (250 mL of 0.1M) Standard Solution of Oxalic Acid

# Our Objective

Preparation of (250 mL of 0.1M) standard solution of oxalic acid.

# The Theory So, it is critical that we can count chemical entities when the entity of interest is a solute dissolved in a solvent, in which case we measure the mass of volume of the solution as a whole (solvent plus all solutes), with volume being the most easily measured. Another common way to represent solution concentration is by molarity. Molar solutions calculate molar concentration in a litre (L) of solution using the Gram Molecular Weight (GMW) of a solute.

Mole Concentration (Molarity): has units of mol/L or M

Moles solute / vol solution=n(moles))/V(L))=M(mol/L)

A substance's Gram Molecular Weight (GMW) (sometimes known as the "formula weight") is the total of the combined atomic weights of all atoms in the molecule given in grams. For example, the GMW of NaCl is equal to the atomic weights of Na (22.99) and Cl (35.45) for a total of 58.44 g.

So for preparing 0.1M solution of Oxalic acid in 250ml the calculation is as follows.

Hydrated oxalic acid = C2H2O4.2H2O

The molecular mass of Oxalic Acid = 126.

12.6 g of oxalic acid per litre of the solution should be dissolved to prepare the M/10 oxalic acid solution.

On the other hand,

12.6 /4 = 3.15 g of crystals of oxalic acid should be dissolved in water and precisely 250 ml of the solution should be produced.

# Learning Outcomes

Students will be able to understand the following:

• What is molality.
• How to prepare the solution for the required experiments if M is given.
• They learn the technique of handling the apparatus and the way of preparing a solution.