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Reactions in Aqueous Solutions

Reactions in Aqueous Solutions. Double-Replacement Reactions in Water. Objectives:. Describe aqueous solutions Write complete ionic and net ionic equations for reactions in aqueous solutions Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas.

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Reactions in Aqueous Solutions

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  1. Reactions in Aqueous Solutions Double-Replacement Reactions in Water

  2. Objectives: • Describe aqueous solutions • Write complete ionic and net ionic equations for reactions in aqueous solutions • Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas

  3. Reactions in Water are Vital… 70% of Earth covered by H2O Your body is 60-70% H2O

  4. Aqueous Solutions • Aqueous from “Aqua” (Latin for water) • Aqueous Solution = Water with stuff dissolved in it • Solute = The stuff that is dissolved • Solvent = The most plentiful substance in the solution • Water = The solvent in an aqueous solution

  5. Solutes • There are many possible solutes—sugar and alcohol are molecular compounds that exist as molecules in aqueous solutions. • Compounds that produce hydrogen ions in aqueous solutions are acids. • Ionic compounds can also be solutes in aqueous solutions. • When ionic compounds dissolve in water, their ions separate in a process called dissociation.

  6. Types of Reactions in aqueous solutions • When two solutions that contain ions as solutes are combined, the ions might react. • If they react, it is always a double replacement reaction. • Three products can form: precipitates, water, or gases

  7. Reactions that form solid precipitates • Aqueous solutions of sodium hydroxide and copper(II) chloride react to form the precipitate copper(II) hydroxide. 2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s) • Ionic equations that show all of the particles in a solution as they actually exist are called complete ionic equations. 2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) → 2Na+(aq) + 2Cl–(aq) + Cu(OH)2(s)

  8. Ions that do not participate in a reaction are called spectator ions and are not usually written in ionic equations. • Formulas that include only the particles that participate in reactions are called net ionic equations: • 2OH–(aq) + Cu2+(aq) → Cu(OH)2(s)

  9. Reactions that produce Water • Some reactions produce more water molecules. • No evidence of a chemical reaction is observable. • HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq) • Without spectator ions:H+(aq) + OH–(aq) → H2O(l)

  10. Reactions that form gases Gases that are commonly produced are carbon dioxide, hydrogen cyanide, and hydrogen sulfide. 2HI(aq) + Li2S(aq)→ H2S(g) + 2LiI(aq)

  11. Reactions that form gases • Another example is mixing an acid and baking soda, which produces carbon dioxide gas: • HCl(aq) + NaHCO3(aq) → H2CO3(aq) + NaCl(aq) • H2CO3(aq) (carbonic acid) decomposes immediately: H2CO3(aq) → H2O(l) + CO2(g)

  12. Combining Reactions • Two reactions can be combined and represented by a single chemical reaction.

  13. Combining Reactions Reaction 1 HCl(aq) + NaHCO3(aq) → H2CO3(aq) + NaCl(aq) Reaction 2 H2CO3(aq) → H2O(l) + CO2(g) Combined equation HCl(aq) + NaHCO3(aq) + H2CO3(aq) → H2CO3(aq) + NaCl(aq) + H2O(l) + CO2(g) Overall equation HCl(aq) + NaHCO3(aq) → H2O(l) + CO2(g) + NaCl(aq)

  14. Baking Soda + Acid This is what makes cakes rise!

  15. Review • Reactions between ionic compounds in water produce a gas, a solid precipitate, or a liquid (H2O, usually) • These reactions are double replacement reactions • Chemists write aqueous reactions as ionic equations – these show the ions dissolved in water and their interactions • A net ionic equation shows only those ions that interact to produce a solid, liquid or gaseous product • You can combine reactions and cancel out the ions and compounds that appear as both reactants and products.

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