Equilibrium in Physical and Chemical Processes Quiz

Acid-Base Classifications

• Arrhenius theory classifies substances as acids or bases based on their ability to donate or accept hydrogen ions (H+)
• Bronsted-Lowry theory expands this definition to include conjugate acid-base pairs and the transfer of protons (H+)
• Lewis theory defines acids as electron pair acceptors and bases as electron pair donors

pH Scale

• The pH scale measures the concentration of hydrogen ions (H+) in a solution
• pH ranges from 0-14, with 7 being neutral, below 7 being acidic, and above 7 being basic

Role of Water

• Water (H2O) can act as an acid or a base, donating or accepting hydrogen ions (H+), making it amphoteric
• Water plays a crucial role in acid-base chemistry, often participating in acid-base reactions as a reactant or solvent

Ionic Product of Water

• The ionic product of water (Kw) represents the equilibrium constant for the self-ionization of water: H2O + H2O ⇌ H3O+ + OH-
• The ionic product of water is 1.0 × 10^(-14) at 25°C

Buffer Solutions

• Buffer solutions resist changes in pH when an acid or base is added, maintaining a relatively constant pH
• Buffer solutions consist of a weak acid and its conjugate base, or a weak base and its conjugate acid, which work together to regulate pH