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pH and pOH definitions

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Terms in this set (15)

  • pH Scale
    A scale ranging from 0 to 14 used to measure acidity or basicity, but can extend beyond this range with high concentrations.
  • pOH
    The negative logarithm of hydroxide ion concentration, related to pH by the equation pH + pOH = 14.
  • Hydronium Ion
    The ion H3O+, formed when water acts as a base and accepts a proton.
  • Hydroxide Ion
    The ion OH-, formed when water acts as an acid and donates a proton.
  • Autoionization
    The process where water molecules react with each other to form hydronium and hydroxide ions.
  • Kw
    The ion product constant for water, equal to 1.0x10^-14 at 25°C, representing the product of hydronium and hydroxide ion concentrations.
  • Strong Electrolyte
    A substance that completely ionizes in solution, such as strong acids and bases.
  • Weak Electrolyte
    A substance that partially ionizes in solution, establishing an equilibrium between reactants and products.
  • Neutral pH
    A pH of 7, indicating equal concentrations of hydronium and hydroxide ions, true at 25°C.
  • Strong Acid
    An acid that completely ionizes in solution, increasing hydronium ion concentration significantly.
  • Strong Base
    A base that completely ionizes in solution, increasing hydroxide ion concentration significantly.
  • Weak Acid
    An acid that partially ionizes in solution, with equilibrium favoring the reactants.
  • Weak Base
    A base that partially ionizes in solution, with equilibrium favoring the reactants.
  • Ion Product
    The product of the concentrations of ions in a solution, such as Kw for water.
  • Bronsted-Lowry Acid
    A substance that donates a proton (H+) in a chemical reaction.