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AP Chemistry Chapter 4 Molarity is moles of solute per liter of solution not per liter of solvent Lecture Outline 4 1 General Properties of Aqueous Solutions

➢ molar solubility—the number of moles of solute that dissolves in exactly 1 0 L of solvent, expressed in units of molarity, M or the use of square brackets ➢

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[PDF] Chapter 4 Aqueous Reactions and Solution Stoichiometry

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Common Student Misconceptions

Molarity is moles of solute per liter of solution not per liter of solvent. Students sometimes used moles instead of molarity in MinitialVinitial = MfinalVfinal. Students sometimes think that water is a good conductor.

Students sometimes have a problem with the arbitrary difference between strong and weak electrolytes.

The symbols

̢ (equilibrium) and (resonance are often confused.

Students often do not see that the net ionic equation for the reaction between strong acids and strong

bases is always H +(aq) + OH -(aq) H 2 O (l) Students try to split polyatomic ions into smaller ions when they write net ionic equations. Students do not appreciate the difference between equivalence point and end point.

Lecture Outline

4.1 General Properties of Aqueous Solutions

• A solution is a homogeneous mixture of two or more substances. • A solution is made when one substance (the solute) is dissolved in another (the solvent). • The solute is the substance that is present in smallest amount. • Solutions in which water is the solvent are called aqueous solutions.

Electrolytic Properties

• All aqueous solutions can be classified in terms of whether or not they conduct electricity.

• If a substance forms ions in solution, then the substance is an electrolyte, and the solution conducts

electricity. Example: NaCl (a)

• If a substance does not form ions in solution, then the substance is a nonelectrolyte, and the solution does

not conduct electricity. Example: sucrose, methanol (b) AP Chemistry Chapter 4. Aqueous Reactions and Solution Stoichiometry - 2 -

Ionic Compounds in Water

• When an ionic compound dissolves in water, the ions are said to dissociate.

• This means that in solution, the solid no longer exists as a well-ordered arrangement of ions in contact

with one another. • Instead, each ion is surrounded by a shell of water molecules.

• This tends to stabilize the ions in solution and prevent cations and anions from recombining.

• The positive ions have the surrounding oxygen atoms of water pointing towards the ion, negative ions

have the surrounding hydrogen atoms of water pointing towards the ion.

• The transport of ions through the solution causes electric current to flow through the solution.

Molecular Compounds in Water

• When a molecular compound (e.g. CH 3 OH ) dissolves in water, there are no ions formed.

• Therefore, there is nothing in the solution to transport electric charge and the solution does not conduct

electricity. • There are some important exceptions. • For example, NH 3 (g) reacts with water to form NH 4+ (aq) and OH (aq). • For example, HCl(g) in water ionizes to form H (aq) and Cl (aq).

Strong and Weak Electrolytes

• Compounds whose aqueous solutions conduct electricity well are called strong electrolytes. • These substances exist only as ions in solution. • Example NaCl:

NaCl(aq) Na

(aq) + Cl (aq) • The single arrow indicates that the Na and Cl ions have no tendency to recombine to form NaCl molecules. • In general, soluble ionic compounds are strong electrolytes. • Compounds whose aqueous solutions conduct electricity poorly are called weak electrolytes • These substances exist as a mixture of ions and un-ionized molecules in solution. • The predominant form of the solute is the un-ionized molecule. • Example: acetic acid, HC 2 H 3 O 2 HC 2 H 3 O 2 (aq) ̢ H (aq) + C 2 H 3 O 2- (aq) • The double arrow means that the reaction is significant in both directions. • It indicates that there is a balance between the forward and reverse reactions. • This balance produces a state of chemical equilibrium.

Sample Exercise 4.1 (p. 116)

The diagram on the left (p. 116) represents an aqueous solution of one of the following compounds: MgCl

KCl, or K

2 SO 4 . Which solution does it best represent?

Practice Exercise 4.1

If you were to draw diagrams (such as that shown on the left of p. 116) representing aqueous solutions of each

of the following ionic compounds, how many anions would you show if the diagram contained six cations?

a) NiSO 4 b) Ca(NO 3 2 c) Na 3 PO 4 d) Al 2 (SO 4 3 AP Chemistry Chapter 4. Aqueous Reactions and Solution Stoichiometry - 3 -

4.2 Precipitation Reactions

• Reactions that result in the formation of an insoluble product are known as precipitation reactions.

• A precipitate is an insoluble solid formed by a reaction in solution. • Example: Pb(NO 3 2 (aq) + 2KI(aq) PbI 2 (s) + 2KNO 3 (aq)

Solubility Guidelines for Ionic Compounds

• The solubility of a substance is the amount of that substance that can be dissolved in a given quantity of

solvent. • A substance with a solubility of less than 0.01 mol/L is regarded as being insoluble. • Experimental observations have led to empirical guidelines for predicting the solubility. • Solubility guidelines for common ionic compounds in water: • Compounds containing alkali metal ions or ammonium ion are soluble. • Compounds containing NO 3- or C 2 H 3 O 2- are soluble. • Compounds containing Cl , Br or I are soluble. • Exceptions: Compounds of Ag , Hg 22+
, and Pb 2+ • Compounds containing SO 42-
are soluble. • Exceptions: Compounds of Sr 2+ , Ba 2+ , Hg 22+
, and Pb 2+ • Compounds containing S 2- are insoluble. • Exceptions: Compounds of NH 4+ , the alkali metal cations, and Ca 2+ , Sr 2+ , and Ba 2+ • Compounds of CO 32-
or PO 43-
are insoluble. • Exceptions: Compounds of NH 4+ and the alkali metal cations. • Compounds of OH are insoluble. • Exceptions: Compounds of the alkali metal cations, and Ca 2+ , Sr 2+ , and Ba 2+ AP Chemistry Chapter 4. Aqueous Reactions and Solution Stoichiometry - 4 -

Sample Exercise 4.2 (p. 118)

Classify the following ionic compounds as soluble or insoluble in water:quotesdbs_dbs17.pdfusesText_23

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