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Reactions in Aqueous Solutions

Reactions in Aqueous Solutions . Ms. Mack Chapter 10, Section 3 Chemistry I- 3/24/09. Introduction. Many reactions involve substances dissolved in water. When this happens, solutions form Solutions (homogeneous substances) Two parts: SOLUTES- substances dissolved in water

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Reactions in Aqueous Solutions

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  1. Reactions in Aqueous Solutions Ms. Mack Chapter 10, Section 3 Chemistry I- 3/24/09

  2. Introduction • Many reactions involve substances dissolved in water. • When this happens, solutions form • Solutions (homogeneous substances) • Two parts: • SOLUTES- substances dissolved in water • SOLVENTS- the most plentiful substance in a solution Water is the "universal solvent"

  3. Water, the universal solvent (H2O) • Examples of Solutes: • Molecular compounds that exist as molecules • Molecular compounds that form ions when they dissolve in water (H+ ions=acids) • Ionic compounds • When dissolved in water, the ions can separate

  4. The Products • When 2 aqueous solutions that contain ions are combined, the ions may react with one another in a DOUBLE-REPLACEMENT reaction producing: A.Precipitate (s) B. Water (l) C. Gas (g)

  5. A. Precipitate • Use ionic equations to show the details of reactions that involve ions in aqueous solutions • Substances are written as ions • Complete ionic equations- show all particles involved in a chemical reaction

  6. Complete Ionic Equation NaCl (aq) + AgNO3 (aq) NaNO3 (aq) + AgCl (s) Complete: Na+(aq) + Cl- (aq) + Ag+ (aq) + NO3-(aq) Na+ (aq) + NO3- (aq) + AgCl (s)

  7. Spectator Ions • Notice, that there are ions that appear on both sides of the equation • These ions do not participate in the formation of the solid product • These ions are called spectator ions. • What were the spectator ions in the previous slide?

  8. Net Ionic Equations • Equations that show only the ions involved- omitting the spectator ions are called complete ionic equations! From the previous example: Cl- + Ag+AgCl (s)

  9. Practice! • Write the chemical, balanced, complete ionic and net ionic equation for the following: Aqueous solutions of potassium iodide and silver nitrate are mixed, forming the precipitate silver iodide. See white board for solution!

  10. B. Water • Some reactions form water • No evidence of the chemical reaction can be observed. Why? • Example: HCl (aq) + KOH (aq) H2O (l) + KCl (aq) H+(aq) + OH-(aq) H2O (l)

  11. Practice! Sulfuric acid (H2SO4) and aqueous potassium hydroxide react to produce water and potassium sulfate.

  12. C. Gas • Common gases produced: carbon dioxide, hydrogen cyanide, and hydrogen sulfide Example: Na2S (aq) + HCl (aq) NaCl (aq) + H2S (g)

  13. Practice! Sulfuric acid and aqueous rubidium sulfide with production of hydrogen sulfide gas

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