Find the normality of oxalic acid solution containing 63 g of crystalline oxalic acid in 500 ml of solution.

To find the normality of an oxalic acid solution, we first need to determine the number of equivalents of the acid present in the solution. Oxalic acid (H₂C₂O₄) is a diprotic acid, meaning it can donate two protons (H⁺) per molecule.

Step 1: Calculate Molar Mass

The molar mass of oxalic acid is calculated as follows:

• Carbon (C): 12.01 g/mol × 2 = 24.02 g/mol
• Hydrogen (H): 1.01 g/mol × 2 = 2.02 g/mol
• Oxygen (O): 16.00 g/mol × 4 = 64.00 g/mol

Total Molar Mass: 24.02 + 2.02 + 64.00 = 90.04 g/mol

Step 2: Calculate Moles of Oxalic Acid

Now, we can find the number of moles of oxalic acid in 63 g:

Moles = Mass (g) / Molar Mass (g/mol)

Moles = 63 g / 90.04 g/mol ≈ 0.699 moles

Step 3: Calculate Equivalents

Since oxalic acid can donate two protons, the number of equivalents is:

Equivalents = Moles × 2

Equivalents = 0.699 moles × 2 ≈ 1.398 equivalents

Step 4: Calculate Normality

Normality (N) is defined as the number of equivalents per liter of solution:

Normality = Equivalents / Volume (L)

Convert 500 ml to liters: 500 ml = 0.5 L

Normality = 1.398 equivalents / 0.5 L = 2.796 N

Final Result

The normality of the oxalic acid solution is approximately 2.80 N.