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The pH Scale definitions

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  • pH Scale
    A numerical range, typically 0 to 14, used to express the acidity or basicity of a solution under standard conditions.
  • Hydrogen Ion Concentration
    A measure, in moles per liter, of H+ present in a solution, directly influencing its acidity.
  • Hydroxide Ion Concentration
    A measure, in moles per liter, of OH- present in a solution, directly influencing its basicity.
  • pOH
    A logarithmic value representing the concentration of hydroxide ions, calculated as the negative log of [OH-].
  • Negative Logarithm
    A mathematical operation used to convert small ion concentrations into manageable numbers for pH and pOH calculations.
  • Neutral Solution
    A state where H+ and OH- concentrations are equal, each at 1.0 x 10^-7 M, resulting in a pH of 7.
  • Basic Solution
    A classification for solutions with pH above 7, where OH- concentration exceeds H+ concentration.
  • Acidic Solution
    A classification for solutions with pH below 7, where H+ concentration exceeds OH- concentration.
  • Ion Product Constant for Water
    A fixed value, 1.0 x 10^-14 at 25°C, representing the product of H+ and OH- concentrations in water.
  • Antilogarithm
    A mathematical process used to reverse a logarithm, allowing calculation of ion concentrations from pH or pOH.
  • Molarity
    A unit expressing the number of moles of solute per liter of solution, used for ion concentrations.
  • Relationship between pH and pOH
    A direct connection where their sum equals 14, enabling calculation of one value if the other is known.
  • Acidity
    A property determined by the relative abundance of H+ ions in a solution, reflected by lower pH values.
  • Basicity
    A property determined by the relative abundance of OH- ions in a solution, reflected by higher pH values.