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Reactions in Aqueous Solutions

Reactions in Aqueous Solutions. Lecture 4. Reactions that form Precipitates. Some reactions that form precipitates include ionic substances that leave ions dissolved in the aqueous solution.

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Reactions in Aqueous Solutions

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  1. Reactions in Aqueous Solutions Lecture 4

  2. Reactions that form Precipitates • Some reactions that form precipitates include ionic substances that leave ions dissolved in the aqueous solution. • These reactions are written using complete ionic equations that show all of the particles in a solution as they really exist. • Ions that do not react are called spectator ions. When these ions are not included in the ionic equation, the equation is a net ionic equation. • Spectator ions are crossed out of the complete ionic equation and only the reacting ions are left in the net ionic equation.

  3. Example • Lithium iodide (aq) + Silver nitrate (aq)  Silver iodide (s) + Lithium nitrate (aq) • LiI (aq) + AgNO3 (aq)  AgI (s) + LiNO3 (aq) • Li+ + I- + Ag+ + NO3-  AgI (s) + Li+ +NO3- • Net Ionic = Ag+ + I-  AgI (s)

  4. Reactions that form Water • These double-replacement reactions produce water in aqueous solutions. • Because water has no color or odor, it is difficult to observe evidence of the reaction. • These reaction equations are written as complete and net ionic equations where the only ions reacting are the hydrogen ions and the hydroxide ions.

  5. Example • Sodium hydroxide (aq) + Hydrochloric acid (aq)  Sodium chloride (aq) + water (l) • NaOH (aq) + HCl (aq)  NaCl (aq) + H2O (l) • Na+ + OH- + H+ + Cl-  Na+ + Cl- + H2O (l) • Net ionic = H+ +OH-  H2O (l)

  6. Reactions that form Gases • This type of double-replacement reaction produces a gas that will bubble to the surface and escape. • The chemical reaction equations are written as complete and net ionic equations. • When one product decomposes upon production, it can be incorporated into the original equation.

  7. Example • Hydrochloric acid (aq) + Sodium sulfate (aq)  Sodium chloride (aq) + Hydrogen sulfate (g) • HCl (aq) + Na2SO4 (aq)  NaCl (aq) + H2SO4 (g) • Balance = 2 HCl (aq) + Na2SO4 (aq)  2 NaCl (aq) + H2SO4(g) • 2 H+ + 2 Cl- + 2 Na+ + SO42-  2 Na++ 2 Cl- + H2SO4(g) • Net = 2 H+ + SO42-  H2SO4(g)

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