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General Approach to Acid-Base Systems definitions

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  • Strong Acid
    A substance that fully dissociates in water, yielding a high concentration of H+ ions and exhibiting a Ka value greater than 1.
  • Strong Base
    A compound that completely ionizes in solution, producing a significant amount of OH- ions and characterized by a Kb value greater than 1.
  • Electrolyte
    A substance that conducts electricity in solution due to the presence of freely moving ions formed upon dissolution.
  • Ionization
    The process by which a molecule separates into ions when dissolved, leading to electrical conductivity in the solution.
  • Ka Value
    A quantitative measure of acid strength, indicating the equilibrium constant for the dissociation of an acid in water.
  • Kb Value
    A numerical expression of base strength, representing the equilibrium constant for the dissociation of a base in water.
  • pH
    A logarithmic scale used to specify the acidity of a solution, calculated as the negative log of the H+ ion concentration.
  • pOH
    A logarithmic measure of the basicity of a solution, determined by taking the negative log of the OH- ion concentration.
  • Autoionization of Water
    A self-ionization process where water molecules generate small amounts of H+ and OH- ions, affecting solution pH at low solute concentrations.
  • Neutral Solution
    A state where the concentrations of H+ and OH- ions are equal, resulting in a pH of 7, typically observed when acid or base is very dilute.
  • Concentration
    The amount of solute present in a given volume of solution, crucial for determining the calculation method for pH or pOH.
  • Negative Logarithm
    A mathematical operation used to convert ion concentrations into pH or pOH values, simplifying the comparison of acidity or basicity.
  • Hydronium Ion
    The H+ ion in aqueous solution, responsible for acidic properties and central to pH calculations.
  • Hydroxide Ion
    The OH- ion in solution, responsible for basic properties and essential for determining pOH.
  • Systematic Approach
    A stepwise method for calculating pH or pOH, especially necessary when acid or base concentrations are between 10^-6 M and 10^-8 M.