8.3 Acid-Base Reactions and Buffers

    Cards (59)

    • The Brønsted-Lowry definition is broader than the Arrhenius definition because it does not require water
    • A Lewis acid accepts an electron pair
    • Brønsted-Lowry bases are proton donors.
      False
    • Brønsted-Lowry acids are proton donors, and Brønsted-Lowry bases are proton acceptors.

      True
    • Match the acid-base definition with its description:
      Arrhenius ↔️ Releases H⁺ in water
      Brønsted-Lowry ↔️ Proton donor or acceptor
      Lewis ↔️ Electron pair acceptor
    • What two products are formed in an acid-base neutralization reaction?
      Salt and water
    • What type of acid is BF₃ according to the Lewis definition?
      Accepts electron pairs
    • What do Brønsted-Lowry acids donate?
      Protons (H⁺)
    • Lewis bases donate electron pairs.

      True
    • Acid-base neutralization reactions form salt and water
    • In the reaction HCl + H₂O ⇌ H₃O⁺ + Cl⁻, what is the conjugate base of HCl?
      Cl⁻
    • A buffer system maintains a stable pH
    • If the concentrations of a weak acid and its conjugate base are equal, the pH is equal to pKₐ
    • According to the Arrhenius definition, acids release H⁺
    • Match the acid-base definition with its key concept:
      Arrhenius ↔️ Releases H⁺ or OH⁻ in water
      Brønsted-Lowry ↔️ Proton donor or acceptor
      Lewis ↔️ Electron pair acceptor or donor
    • What are the products of the reaction between HCl and NaOH?
      NaCl and H₂O
    • What is the conjugate base of HCl in the reaction with water?
      Cl⁻
    • Conjugate acid-base pairs differ by a single proton
    • What are the two types of mixtures that form a buffer system?
      Weak acid/conjugate base or weak base/conjugate acid
    • The Henderson-Hasselbalch equation relates pH to pKa and the ratio of conjugate base
    • What is the Arrhenius definition of an acid?
      Releases H⁺ in water
    • What is the Lewis definition of a base?
      Donates electron pair
    • Give an example of an Arrhenius acid.
      HCl
    • In the reaction between HCl and NaOH, H⁺ ions from HCl combine with OH⁻ ions from NaOH to form H₂O
    • What do Arrhenius acids release in water?
      Hydrogen ions (H⁺)
    • An example of a Brønsted-Lowry base is H₂O
    • Match the acid-base theory with its definition:
      Arrhenius ↔️ Releases H⁺ or OH⁻ in water
      Brønsted-Lowry ↔️ Donates or accepts H⁺
      Lewis ↔️ Accepts or donates electron pairs
    • Neutralization reactions involve the combination of H⁺ and OH⁻ ions.

      True
    • Conjugate acid-base pairs differ by a single proton (H⁺).

      True
    • The Henderson-Hasselbalch equation relates pH to pKₐ and the ratio of conjugate base to acid concentrations.

      True
    • The pH of the buffer is 4.76
    • NaOH is an example of an Arrhenius base

      True
    • The Lewis definition is the most general
    • In a neutralization reaction, an acid donates H⁺
    • A buffer system resists changes in pH
    • What does HCl become after donating a proton?
      Cl⁻
    • Acetic acid (CH₃COOH) is an example of a weak acid
    • What is the Henderson-Hasselbalch equation?
      pH = pK_a + \log \frac{[A^-]}{[HA]}</latex>
    • Factors influencing buffer capacity
      1️⃣ Concentration of components
      2️⃣ Ratio of acid and conjugate base concentrations
    • Buffers are used in industrial processes to ensure product quality by controlling pH.

      True
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