Section 8.1 Water and Chemical Reactions The reactions that are most important to us happen in water. Ex.: Metabolic reactions happen in a watery environment.

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Section 8.1 Water and Chemical Reactions The reactions that are most important to us happen in water. Ex.: Metabolic reactions happen in a watery environment (inside or outside cells) Ex.: Oxygen dissolves in blood (mostly water) and binds to hemoglobin on red blood cells so it can be distributed to body cells; oxygen is used to release energy from food in a series of reactions.

Copyright© by Houghton Mifflin Company. All rights reserved.2 What are the driving forces that cause chemical reactions to happen? Several “tendencies” drive reactants to form products: Formation of a solid Formation of water Transfer of electrons Formation of a gas

Formation of a Solid: Precipitation Reaction A solid forms  new substance formed  chemical reaction has happened A common form of precipitation is the formation of a solid ionic compound from a mixture of two aqueous compounds The solubility of the new compound determines whether a precipitate forms

Copyright© by Houghton Mifflin Company. All rights reserved.4 Formation of solid AgCl (precipitation) from a mixture of KCl and AgNO 3 Solid/powder = precipitate

Copyright© by Houghton Mifflin Company. All rights reserved.5 1.Ions from an ionic compound dissociate (separate) when mixed in water. 2.A new combination of ions (cation and anion) may form. 3.If the new compound is insoluble in water, it will precipitate as a solid.

Possible Ion Combinations (not in notes): Copyright© by Houghton Mifflin Company. All rights reserved.6 Cl - NO 3 - K+K+ KClKNO 3 Ag + AgClAgNO 3 Reactants: KCl and KCl and AgNO 3 Possible new compounds: AgCl and KNO 3 Which of these is insoluble in water?

Copyright© by Houghton Mifflin Company. All rights reserved.7 Using solubility rules: Solubilities of common compounds

8 Predicting the Products of a Precipitation Reaction 1. Write proper, neutral formulas -- consider the products that could form by exchanging the ions of the added salts; 2. Balance the equation using coefficients; 3. Add physical states -- use the solubility rules to decide whether a solid forms and predict its identity.

Equations Used to Describe a Precipitation Reaction Ex.: Precipitation of Silver Chloride Molecular Equation – shows overall reaction with molecular formulas: AgNO 3(aq) + KCl (aq)  AgCl (s) + KNO 3(aq) Complete Ionic Equation – shows strong electrolytes (aq) as ions: Ag + (aq) + NO 3 - (aq) + K + (aq) + Cl - (aq)  AgCl (s) + K + (aq) + NO 3 - (aq) Net Ionic Equation – shows only the components that form the precipitate; spectator ions are not shown: Ag + (aq) + Cl - (aq)  AgCl (s)