Ionic Equilibrium

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An Arrhenius acid is a substance that produces H⁺ ions when dissolved in water. Example: HCl (hydrochloric acid) HCl(aq) → H⁺(aq) + Cl⁻(aq) The H⁺ ion actually binds with water to form hydronium ion

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A conjugate acid-base pair consists of two species that differ by the gain or loss of one proton (H⁺). In the reaction: NH₃ + H₂O ⇌ NH₄⁺ + OH⁻ Conjugate pairs: 1. NH₃/NH₄⁺ (NH₃ is base, NH₄⁺ is its

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For the equilibrium: HA(aq) + H₂O(l) ⇌ H₃O⁺(aq) + A⁻(aq) Kₐ = [H₃O⁺][A⁻]/[HA] Where: • [HA] = concentration of undissociated acid • [H₃O⁺] = concentration of hydronium ions • [A⁻] = concentration of

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For weak acid HA with initial concentration c and degree of dissociation α: At equilibrium: [HA] = c(1-α) [H₃O⁺] = [A⁻] = cα Kₐ = [H₃O⁺][A⁻]/[HA] = (cα)(cα)/c(1-α) = c²α²/c(1-α) = cα²/(1-α) For ver

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Kw is the ionic product constant of water representing auto-ionization: H₂O + H₂O ⇌ H₃O⁺ + OH⁻ Kw = [H₃O⁺][OH⁻] = 1.0 × 10⁻¹⁴ mol²dm⁻⁶ at 25°C In pure water: [H₃O⁺] = [OH⁻] = 1.0 × 10⁻⁷ mol dm⁻³ T

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pH = -log₁₀[H₃O⁺] For 0.01 M HCl: HCl is a strong acid, so it ionizes completely: HCl(aq) → H⁺(aq) + Cl⁻(aq) [H₃O⁺] = 0.01 M = 1.0 × 10⁻² M pH = -log₁₀(1.0 × 10⁻²) = -(-2.0) = 2.0 The solution is

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pH + pOH = pKw = 14 (at 25°C) Solution classification: • Neutral solution: pH = 7, [H₃O⁺] = [OH⁻] • Acidic solution: pH < 7, [H₃O⁺] > [OH⁻] • Basic solution: pH > 7, [H₃O⁺] < [OH⁻] If pH is known: p

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Common ion effect: The suppression of ionization of a weak electrolyte by the addition of a salt containing a common ion. Example: CH₃COOH + CH₃COONa mixture CH₃COOH(aq) ⇌ H⁺(aq) + CH₃COO⁻(aq) CH₃CO