Acid-Base Reaction Buffer Steps

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4 Terms

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Strong Acid and Strong Base

When a strong acid and a strong base are mixed, they react quantitatively in a reaction represented by the equation:

  • H+ (aq) + OH– (aq) → H2O (l)

pH determined by concentration of excess reagent

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Weak Base-Strong Acid

  • If the weak base is in excess, then a buffer solution is formed, and the pH can be determined from the Henderson–Hasselbalch equation equation:

    pOH = pKb + log [B]/[BH+]

  • If the strong acid is in excess, then the pH can be determined from the moles of excess hydronium ion and the total volume of solution

pH = -log10[H3O+]

  • If they are equimolar, then the (slightly acidic) pH can be determined from the equilibrium represented by the equation:

HB+ (aq) + H2O (l) ⇌ B (aq) + H3O+ (aq)

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Strong Base-Weak Acid

  • If the weak acid is in excess, then a buffer solution is formed, and the pH can be determined from the Henderson-Hasselbalch equation

pH = pKa + log[A-]/[HA]

  • If the strong base is in excess, then the pH can be determined from the moles of excess hydroxide ion and the total volume of solution

  • If they are equimolar, then the (slightly basic) pH can be determined from the equilibrium represented by the equation:


A– (aq) + H2O (l) ⇌ HA (aq) + OH– (aq)

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Weak Acid-Weak Base

  • In an acid base reaction, the equilibrium will favour the side with the weaker acid and weaker base

  • If the equilibrium constant for the reaction is greater than one (K >1) the equilibrium will favour the formation of products

    • This means the weaker acid and weaker base are on the product side

  • If the equilibrium constant for the reaction is less than one (K <1) the equilibrium will favour the formation of reactants

    • This means the weaker acid and weaker base are on the reactant side