Skip to main content
Back

Weak Acid-Base Equilibria definitions

Control buttons has been changed to "navigation" mode.
1/15
  • Weak Acid
    A substance with a Ka less than 1 that partially ionizes in water, establishing an equilibrium with its conjugate base and hydronium ion.
  • Acid Ionization Constant
    A value expressing the equilibrium ratio of products to reactants for the dissociation of a weak acid in water.
  • pH
    A logarithmic measure of hydronium ion concentration, calculated as the negative log of [H3O+].
  • Hydronium Ion
    The ion formed when a proton associates with a water molecule, central to acid-base equilibrium calculations.
  • Equilibrium Expression
    A mathematical relationship showing the ratio of product and reactant concentrations at equilibrium for a chemical reaction.
  • Formal Concentration
    The initial molarity of a solute before any reaction or dissociation occurs in solution.
  • ICE Chart
    A tabular method for tracking initial, change, and equilibrium concentrations in chemical reactions.
  • Conjugate Base
    The species formed when a weak acid donates a proton during dissociation in water.
  • Aqueous Solution
    A homogeneous mixture where water acts as the solvent for dissolved substances.
  • pOH
    A logarithmic measure of hydroxide ion concentration, related to pH and used in base calculations.
  • Hydroxide Ion
    The negatively charged ion produced when a base dissociates in water, central to base equilibria.
  • Equilibrium
    The state in a reversible reaction where the rates of forward and reverse processes are equal, stabilizing concentrations.
  • Bronsted-Lowry Definition
    A concept describing acids as proton donors and bases as proton acceptors in chemical reactions.
  • Product
    A substance formed as a result of a chemical reaction, present on the right side of a chemical equation.
  • Reactant
    A starting material in a chemical reaction, present on the left side of a chemical equation.