8.3 Acid-Base Reactions and Buffers

• 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