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Solubility Rules definitions

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  • Solubility
    A chemical property describing how much of a substance can dissolve in a solvent to form a homogeneous mixture.
  • Solute
    A substance that is dissolved in a solvent, often breaking into ions if soluble.
  • Solvent
    A medium, typically a liquid like water, in which other substances are dissolved.
  • Solution
    A uniform mixture formed when a solute dissolves completely in a solvent.
  • Aqueous Ion
    A charged particle surrounded by water molecules after a soluble compound dissociates.
  • Precipitate
    A solid formed when an insoluble compound results from mixing solutions.
  • Group 1A Elements
    Alkali metals like sodium and potassium, whose compounds are always soluble in water.
  • Acetate
    An ion, C2H3O2−, whose compounds are generally soluble with no exceptions.
  • Nitrate
    An ion, NO3−, that forms soluble compounds without exceptions.
  • Ammonium
    A polyatomic ion, NH4+, that ensures solubility when present in ionic compounds.
  • Halogens
    Group 7A elements like chlorine and bromine, usually forming soluble salts except with silver, lead, or mercury.
  • Sulfate
    An ion, SO4^2−, forming soluble salts except with calcium, barium, strontium, silver, or lead.
  • Carbonate
    An ion, CO3^2−, whose compounds are generally insoluble except with Group 1A or ammonium.
  • Hydroxide
    An ion, OH−, usually forming insoluble compounds except with calcium, barium, or strontium.
  • Phosphate
    An ion, PO4^3−, typically resulting in insoluble compounds unless paired with Group 1A or ammonium.