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

Question

Dr. Abubacker · Accepted Answer

[Solution from source] α = √(Ka/C) = √(1.00 × 10⁻⁵/0.100) = 1.00 × 10⁻², i.e. 1.00%. 0.100% would come from Ka/C without the square root. Answer (1).

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

Explanation

Reviewed by Dr. Abubacker

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