Conduct an investigation to determine solubility rules, and predict and analyse the composition of substances when two ionic solutions are mixed

Equilibrium and Acid Reactions > Solution Equilibria >

The following are the solubility rules for common ionic solids. If there two rules appear to contradict each other, the preceding rule takes precedence.

1. Salts containing Group I elements (Li⁺, Na⁺, K⁺, Cs⁺, Rb⁺) are soluble . There are few exceptions to this rule. Salts containing the ammonium ion (NH₄⁺) are also soluble.
2. Salts containing nitrate ion (NO₃^–) are generally soluble.
3. Salts containing Cl ^–, Br ^–, or I ^–are generally soluble. Important exceptions to this rule are halide salts of Ag⁺, Pb²⁺, and (Hg₂)²⁺. Thus, AgCl, PbBr₂, and Hg₂Cl₂ are insoluble.
4. Most silver salts are insoluble. AgNO₃and Ag(C₂H₃O₂) are common soluble salts of silver; virtually all others are insoluble.
5. Most sulfate salts are soluble. Important exceptions to this rule include CaSO₄, BaSO₄, PbSO₄, Ag₂SO₄and SrSO₄ .
6. Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al³⁺are insoluble. Thus, Fe(OH)₃, Al(OH)₃, Co(OH)₂ are not soluble.
7. Most sulfides of transition metals are highly insoluble, including CdS, FeS, ZnS, and Ag₂ Arsenic, antimony, bismuth, and lead sulfides are also insoluble.
8. Carbonates are frequently insoluble. Group II carbonates (CaCO₃, SrCO₃, and BaCO_​3) are insoluble, as are FeCO₃and PbCO₃.
9. Chromates are frequently insoluble. Examples include PbCrO₄and BaCrO₄.
10. Phosphates such as Ca₃(PO₄)₂ and Ag₃PO₄are frequently insoluble.
11. Fluorides such as BaF₂, MgF₂, and PbF₂are frequently insoluble.

These rules are based on the following definitions of the terms soluble, insoluble, and slightly soluble.

–potassium chloride and silver nitrate

The reaction between potassium chloride and silver nitrate would result in the formation of silver chloride which is a white precipitate.

– potassium iodide and lead nitrate

When you combine lead nitrate and potassium iodide solutions, a double-replacement reaction happens. The two compounds react, and the positive ions and negative ions of the two reactants switch places, creating two new compounds Lead particles and iodide particles combine and create two new compounds, a yellow solid called lead iodide and a white solid called potassium nitrate.

– sodium sulfate and barium nitrate

Barium nitrate and sodium sulphate react together to form one soluble salt, sodium nitrate, and an insoluble salt, barium sulphate. Barium sulphate is one of the most insoluble compounds known.