How do I make 0.1 N H2SO4?

To prepare a 0.1 Normal (0.1 N) H₂SO₄ solution, you need to consider the equivalent weight of sulphuric acid.

Step 1: Understand normality

For H₂SO₄:

• It is a dibasic acid (gives 2 H⁺ ions)
• Molecular weight = 98 g/mol
• Equivalent weight = 98 / 2 = 49 g/equiv

Step 2: Calculate required amount

Normality formula:
N = equivalents / liter

For 0.1 N:

Required = 0.1 × 49 = 4.9 g per liter

Step 3: Preparation

• Take about 500 mL distilled water
• Add 4.9 g of H₂SO₄ (or equivalent volume of concentrated acid)
• Mix carefully (always add acid to water)
• Make up the volume to 1 liter

If using concentrated acid:

• Use dilution formula: N₁V₁ = N₂V₂
• Concentrated H₂SO₄ = 36 N

So,

36 × V₁ = 0.1 × 1000

V₁ = 2.78 mL

Final Answer:

To prepare 0.1 N H₂SO₄, use 4.9 g per liter or -2.78 mL concentrated acid diluted to 1 L

Key Takeaway:

Normality depends on equivalent weight, and for H₂SO₄ (dibasic), it is 49 g/equiv.