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Solubility Rules

Solubility Rules. Precipitation Reactions. If you’re not part of the solution You’re part of the precipitate. Types of reactions. Single Replacement Double Replacement Synthesis Decomposition Combustion NEW-Precipitation. Precipitation Reaction.

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Solubility Rules

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  1. Solubility Rules

  2. Precipitation Reactions If you’re not part of the solution You’re part of the precipitate

  3. Types of reactions • Single Replacement • Double Replacement • Synthesis • Decomposition • Combustion • NEW-Precipitation

  4. Precipitation Reaction • Reaction where two soluble salts react to form an insoluble salt. • Reaction looks like a double replacement reaction.

  5. Solubility Rules • Some ions always form water soluble compounds. • Other ions always form water insoluble compounds • The rest are sometimes water soluble and sometimes insoluble

  6. Always Soluble • The following ions are always soluble, no matter what the other ion is. • Group IA (Li, Na…) • Ammonium (NH4+) • Nitrates (NO3-) • Chlorates (ClO3-) • Acetates (C2H3O2-)

  7. Almost always soluble • Halides (Cl, Br…) • Except for fluorides • Except for silver, mercury(I) and lead • Sulfates • Except for barium, calcium, lead, mercury(I)

  8. Mostly insoluble • Hydroxide (OH-) • Except for barium, strontium and calcium (these ARE soluble along with the always soluble ions) • Sulfides, carbonates, chromates, and phosphates.

  9. Soluble salts • Soluble salts are broken into their ions when in solution. • This means that if two soluble salts are mixed and only soluble salts can be produced, THERE WILL BE NO REACTION

  10. What this means… • For precipitation reactions, the insoluble salts are the ones to look for. • When looking for a possible precipitate, cross out any ions that are always soluble

  11. Example • AgNO3(aq) + NaCl(aq)-> ? • (aq) means the salts are both soluble. • Cross out the always soluble ions • Can the remaining ions be combined to make an insoluble salt? • AgCl is insoluble • So there is a reaction. Halides are mostly soluble except for silver, lead, and mercury

  12. Another example • LiNO3(aq) + FeCl(aq)-> ? • Again, both are dissolved in water • Cross out the always soluble • The iron(I) nitrate will be soluble and lithium chloride will be soluble. • Since no insoluble salt can be formed, NO REACTION

  13. Yet another Sulfates are mostly soluble except for barium, lead, mercury and calcium • CuSO4(aq) + BaCl2(aq)-> ? • Cross out the always soluble • Oops, nothing is always soluble. • Look for anything that is mostly insoluble. • Look for anything that can cause it to be insoluble • There will be a reaction • The precipitate will be barium sulfate

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