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Aqueous Solutions and Ionic Equations: Understanding Reactivity

Learn how to write Ionic Equations for reactions in aqueous solutions and predict precipitates using precipitation diagrams. Understand spectator ions and net ionic equations.

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Aqueous Solutions and Ionic Equations: Understanding Reactivity

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  1. Aqueous Solutions Write what is in the purple boxes

  2. Ionic Equations • When a soluble substance is dissolved in water, the substance often breaks into ions. This solution is said to be an aqueous solution. • Pb(NO3)2(aq) Pb2+(aq)+ 2NO3-(aq) • NaI(aq)  Na+(aq)+ I-(aq) An aqueous solution is ions dissolved in water

  3. Ionic Equations • Consider the reaction… • Pb(NO3)2(aq) + 2NaI(aq) PbI2(s) + 2NaNO3(aq) • What is really going on is… • Pb2+ + 2NO3- + 2Na+ + 2I- PbI2(s) + 2Na+ + 2NO3- • Note that the Na+ ion and the NO3- ion are not reacting. They are said to be spectator ions.

  4. Net Ionic Equations • It is often useful to write an equation showing only the species that are actually reacting. This is called a net ionic equation. It does not show the spectator ions. Pb2+ + NO3- + Na+ + 2I- PbI2(s) + Na+ + NO3- becomes…. Pb2+(aq)+ 2I-(aq) PbI2(s)

  5. Precipitates • The solid formed from mixing two aqueous solutions is called the precipitate

  6. To predict precipitates, use the Precipitation Diagram A solid box means a solid forms

  7. Examples • NaOH(aq) + Cu(NO3)2(aq) • Na3PO4(aq) + Fe(NO3)3(aq) • MgSO4(aq) + AgNO3(aq) • KOH(aq) + NaNO3(aq)

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