Properties of Compounds in Aqueous Solution - Chemistry

Chemistry 112

Chapter 5-Kotz

Fetzer Gislason

Properties of Compounds in Aqueous Solution

Aqueous solutions: a solution is a homogeneous mixture of pure substances. We can distinguish the type

of substance in solution by checking to see if the solution conducts electricity or not.

? Substances are called electrolytes if their water solution conducts electricity.

Strong electrolytes: ionic compounds, strong bases and strong acids

weak electrolytes: weak acids and weak bases.

? Substances are called nonelectrolytes if their water solution does not conduct electricity.

nonelectrolytes: Molecular compounds.

Ionic compounds in water solution dissociate into their ions. Ionic compounds generally contain a

metal and a nonmetal or a metal and a polyatomic ion.

Mg(C2H3O2)2

Ba3(PO4)2

5.2 Precipitation Reactions: the formation of a solid when two solutions are mixed. (page 171) a) AgNO3(aq) + NaCl(aq)

b) (NH4)2CO3(aq) + Cd(NO3)2

c) A solution of sodium sulfate is added to a solution of potassium nitrate. Write the net ionic equation for this.

[In a precipitate reaction, the net ionic equation includes only those ions that make up the precipitate.] 5.3 Acid-base reactions: The Bronsted-Lowry theory defines an acid as a proton donor; a base is a proton acceptor. HCl + H2O H3O+ + ClHCl + NH3 NH4+ + Cl-

Strong acids ionize all of their H+. Strong acids are strong electrolytes. (Table 5.2 lists strong acids and strong bases.) Memorize this.

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Chemistry 112

Chapter 5-Kotz

Fetzer Gislason

Weak acids ionize only some of their H+ ions. Weak acids are weak electrolytes.

HC2H3O2 + H2O

Classify the following as either strong or weak electrolytes: HClO4, HClO2, LiOH, NH3

Classify the following as either strong or weak electrolytes: H2SO3 , C2H5OH, KClO3, Cu(NO3)2, HBrO, KOH, C12H22O11

Acids can be monoprotic (HF), diprotic (H2SO4), triprotic (H3PO4) Acid-base Neutralization reactions: acid + base salt + water HCl + NaOH Cr(OH)3 + HNO3 5.5 Gas-forming Reactions:

5.6 Classifying reactions in aqueous solution

Reaction type Precipitation Acid-base neutralization Gas forming Oxidation-reduction

Driving Force Formation of an insoluble compound Formation of molecular water Evolution of a water-insoluble gas Electron transfer

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