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A weak acid, HA, has a Ka of 1.00 × 10⁻⁵. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to:

1. 1.00%
2. 99.9%
3. 0.100%
4. 99.0%

Correct answer: 1.00%

Solution

The dissociation of the weak acid can be calculated using the formula for percent dissociation: % dissociation = (√(Ka/C) × 100). Substituting Ka = 1.00 × 10⁻⁵ and C = 0.100 mol/L, we get % dissociation ≈ 1.00%.

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