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Ka and Kb of compounds definitions

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  • Weak Acid
    A substance that partially donates protons in water, establishing an equilibrium with limited product formation.
  • Weak Base
    A substance that partially accepts protons in water, resulting in an equilibrium with minimal product formation.
  • Ka
    A measure of the extent a weak acid dissociates in water, indicating acid strength; values are less than 1 for weak acids.
  • Kb
    A measure of the extent a weak base accepts protons in water, indicating base strength; values are less than 1 for weak bases.
  • Equilibrium Constant
    A ratio of product to reactant concentrations at equilibrium, excluding solids and liquids, specific for each reaction.
  • Acid Dissociation Constant
    A specific equilibrium constant quantifying the ionization of a weak acid in water.
  • Base Dissociation Constant
    A specific equilibrium constant quantifying the ionization of a weak base in water.
  • Kw
    The ion product constant for water, equal to 1.0×10⁻¹⁴ at 25°C, linking Ka and Kb.
  • pKa
    A logarithmic value inversely related to acid strength; lower values indicate stronger acids.
  • pOH
    A logarithmic measure related to hydroxide ion concentration, useful for weak base calculations.
  • Equilibrium Expression
    A mathematical formula showing the ratio of product to reactant concentrations for a reversible reaction.
  • Bronsted-Lowry Theory
    A concept describing acids as proton donors and bases as proton acceptors in chemical reactions.
  • Ion Product Constant
    A fixed value representing the product of hydrogen and hydroxide ion concentrations in water at a given temperature.
  • H3O+
    The hydronium ion formed when an acid donates a proton to water, central to acid-base equilibria.
  • OH−
    The hydroxide ion produced when a base accepts a proton from water, central to base equilibria.