Equilibrium in Physical and Chemical Processes Quiz

Study Notes

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

Description

Test your knowledge on equilibrium in physical and chemical processes with this quiz. Identify the dynamic nature of equilibrium, state the law of equilibrium, explain characteristics of equilibria, write expressions for equilibrium constants, and establish a relationship between Kp and Kc.