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Reactions

Reactions. • Electrolytes, non-electrolytes and weak electrolytes. Ionic solutions can be identified by their ability to conduct electricity. If a large number of ions are present in a solution, the solution will be an excellent conductor of electricity.

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Reactions

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  1. Reactions

  2. • Electrolytes, non-electrolytes and weak electrolytes • Ionic solutions can be identified by their ability to conduct electricity. • If a large number of ions are present in a solution, the solution will be an excellent conductor of electricity. • Such a substance is completely ionized and is a strong electrolyte. All soluble ionic compounds, but very few molecular compounds are strong electrolytes.

  3. • Electrolytes, non-electrolytes and weak electrolytes • If the solution conducts electricity only weakly, there is likely to be only a few ions present. Such a substance is partially ionized and is a weak electrolyte. • Non-electrolytes have no ions present in solution and therefore cannot conduct electricity. • Such a substance is NOT ionized and is a non-electrolyte. Most molecular compounds are either nonelectrolytes or weak electrolytes

  4. Net Ionic Equation • Net ionic equation: a chemical equation that shows only ions or pure substances that are changed in the reaction • Spectator ion: an ion that remains in solution and does not participate in a chemical reaction

  5. Net Ionic Equation • If you mixed aqueous solutions of calcium chloride (CaCl2 (aq)) and sodium nitrate (NaNO3 (aq)), you might be tempted to predict that the following chemical reaction would occur: CaCl2 (aq) + 2NaNO3 (aq) Ca(NO3)2 (aq) + 2NaCl (aq)

  6. Dissociation occurs:

  7. Detailed Ionic Equation • This means that what we really have in the beaker is: Ca2+ (aq) + Cl− (aq) + Na+ (aq) + NO3− (aq)  Ca2+ (aq)  +  NO3− (aq) + Na+ (aq) + Cl− (aq) • Did a reaction occur?

  8. Detailed Ionic Equation • Now consider the reaction of aqueous silver nitrate with aqueous sodium carbonate: • AgNO3 (aq) + Na2CO3 (aq)  Ag2CO3 (s) + NaNO3 (aq) • What is different about this reaction?

  9. Detailed Ionic Equation • The detailed ionic equation would look like this: • Ag+ (aq) + NO3− (aq) + Na+ (aq) + CO32− (aq)  Ag2CO3 (s) + Na+ (aq) + NO3− (aq) • If we cancel out the spectator ions… • What would be left?

  10. Net Ionic Equation • we are left with the unbalancednet ionic equation for this reaction: Ag+ (aq) + CO32− (aq)  Ag2CO3 (s) • The balancednet ionic equation would therefore be: 2 Ag+ (aq) + CO32− (aq)  Ag2CO3 (s)

  11. Strong acids and bases are written in ionic form; weak acids and bases are written in molecular form • Polyprotic Acids: The second and subsequent ionizations are always weak, whether or not the original is strong or weak. • Soluble Salts are written in ionic form • Insoluble Salts are written in the molecular form • Solids, liquids and gases are always written in molecular form.

  12. Solubility Rules

  13. Predict if a reaction takes place between the following solutions. If it does, write a net ionic equation for the reaction. • KOH(aq) + MgBr2(aq) → • BaS(aq) + NiSO4(aq) → • (NH4)2SO4(aq) + ZnCl2(aq) → • AlCl3(aq) + LiOH(aq) →

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