In how many litres of water, 10 g of `CH_3COOH` should be dissolved to give `[H] = 10^(-3)? K_a(CH_3COOH) = 1.8 xx 10^(-5)`?

Explanation

To solve the problem, we need to determine how many liters of water are required to dissolve 10 g of acetic acid (CH₃COOH) to achieve a hydrogen ion concentration of [H⁺] = 10⁻³ M, given that the dissociation constant (Kₐ) for acetic acid is 1.8 × 10⁻⁵.

### Step-by-Step Solution:

1. **Calculate the Molar Mass of Acetic Acid (CH₃COOH)**:
- The molecular formula of acetic acid is CH₃COOH.
- The molar mass can be calculated as follows:
- C: 12.01 g/mol (2 carbon atoms)
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