Question

Determine the volume of HCl required to prepare 0.6 N HCl solution (Given: specific gravity of HCl = 1.18 g/ml; purity percentage = 35%)

• A. 6.50 ml
• B. 53.03 ml
• C. 73.83 ml
• D. 65.10 ml

Hint:

Acid dilution calculation:
- Normality of concentrated acid = (Sp. Gr. × Purity × 1000) Eq. wt.
- Use N₁V₁ = N₂V₂ for dilution.

Answer 1

The Correct Option is B

Step 1: Understanding the Question:
This question tests the calculation of the volume of concentrated acid needed to prepare a dilute solution.

Step 2: Key Formula or Approach:
Normality of concentrated HCl = (Specific gravity × Purity × 1000) Equivalent weight.
Equivalent weight of HCl = 36.5 gequiv.
Then use the dilution formula: N₁V₁ = N₂V₂.

Step 3: Detailed Explanation:
Given:
Specific gravity = 1.18 g/ml.
Purity = 35% = 0.35.
Equivalent weight of HCl = 36.5 gequiv.
Normality of concentrated HCl = (1.18 × 0.35 × 1000) 36.5 = 11.31 N.
Assume we need to prepare 1 L (1000 ml) of 0.6 N HCl.
N₁V₁ = N₂V₂ → 11.31 × V₁ = 0.6 × 1000.
V₁ = (0.6 × 1000) 11.31 = 53.03 ml.
Thus, 53.03 ml of concentrated HCl is required.
Final Answer:
Thus, the volume required is 53.03 ml, which corresponds to option (B).
[0.5cm]