How to Predict if a Compound is Soluble Using Solubility Rules

Learn how to predict compound solubility with key solubility rules for nitrates, acetates, alkali metals, halides, and sulfates.

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To predict if a compound is soluble, use the solubility rules: 1. Most nitrates (NO3-) and acetates (CH3COO-) are soluble. 2. Compounds containing alkali metal ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) are generally soluble. 3. Chlorides (Cl-), bromides (Br-), and iodides (I-) are soluble, except when paired with Ag+, Pb2+, or Hg2+. 4. Sulfates (SO42-) are soluble, with exceptions like BaSO4, PbSO4, and SrSO4. Insolubility can often be assumed for most carbonates (CO32-), phosphates (PO43-), sulfides (S2-), and hydroxides (OH-), except for those of the alkali metals and NH4+.

FAQs & Answers

  1. What are the general solubility rules for ionic compounds? Most nitrates and acetates are soluble; alkali metal and ammonium ions typically form soluble compounds; halides are soluble except with Ag+, Pb2+, and Hg2+; sulfates are soluble with some exceptions like BaSO4 and PbSO4.
  2. Which compounds are usually insoluble in water? Most carbonates, phosphates, sulfides, and hydroxides are insoluble, except when combined with alkali metals or ammonium ions.
  3. Why are some halides insoluble despite general solubility? Halides like chlorides, bromides, and iodides are typically soluble, but when paired with ions such as silver (Ag+), lead (Pb2+), or mercury (Hg2+), they become insoluble due to the formation of precipitates.

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