What is would be the molality of a solution obtained by mixing equal volumes of 30% by weight `H_(2) SO_(4) (d = 1.218 g mL^(-1))` and 70% by weight `H_(2) SO_(4) (d = 1.610 g mL^(-1))`? If the resulting solution has density `1.425 g mL^(-1)`, calculate its molality.

Explanation

To find the molality of the solution obtained by mixing equal volumes of 30% by weight H₂SO₄ (density = 1.218 g/mL) and 70% by weight H₂SO₄ (density = 1.610 g/mL), we can follow these steps:

### Step 1: Calculate the mass of each solution
Assume we take a volume \( V \) mL of each solution.

**For the 30% H₂SO₄ solution:**
- Density = 1.218 g/mL
- Mass = Density × Volume = \( 1.218 \, \text{g/mL} \times V \, \text{mL} = 1.218V \, \text{g} \)
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