1. Chapter 13 – Ions in Aqueous Solutions and Colligative Properties
This chapter is part of the foundational knowledge to understand how acids work (Chapter 14). This chapter is relatively short (Test on Tuesday, March 28) Colligative Property: a property that is determined by the number of particles present in a system, but that is independent of the properties of the particles themselves.

2. Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation
Dissociation is separation of ions that occurs when an ionic compound dissolves.
1 mol 1 mol 1 mol
1 mol 1 mol 2 mol

3. How can we determine if dissociation will occur?
Chapter 13
How can we determine if dissociation will occur?
What trend do you notice in the following information?
Compound/Molecule
Dissociation Occurs
NaCl
Yes
C6H12O6 No KF
CH4
NO2

4. Chapter 13 Dissociation of NaCl
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation of NaCl

5. Dissociation, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued
Sample Problem A
Write the equation for the dissociation of aluminum sulfate, Al2(SO4)3 , in water. How many moles of aluminum ions and sulfate ions are produced by dissolving 1 mol of aluminum sulfate? What is the total number of moles of ions produced by dissolving 1 mol of aluminum sulfate?

6. Dissociation, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued
Sample Problem A Solution
Given: amount of solute = 1 mol Al2(SO4)3
solvent identity = water
Unknown: a. moles of aluminum ions and sulfate ions
b. total number of moles of solute ions produced
Solution:

7. Dissociation (dissolution)
Write the equation for the dissociation of the following in water, and then determine the number of moles of each ion produced as well as the total number of moles of ions produced.,
a. 1 mol of ammonium chloride
b. 1 mol of sodium sulfide
c. 0.5 mol barium nitrate

8. Dissociation, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued
Precipitation Reactions
Although no ionic compound is completely insoluble, compounds of very low solubility can be considered insoluble for most practical purposes.

9. Soluble and Insoluble Ionic Compounds
Section 1 Compounds in Aqueous Solution
Chapter 13
Soluble and Insoluble Ionic Compounds

10. Particle Model for the Formation of a Precipitate
Section 1 Compounds in Aqueous Solution
Chapter 13
Particle Model for the Formation of a Precipitate

11. Dissociation, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued
Net Ionic Equations
A net ionic equation includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution.
Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction are spectator ions.

12. Dissociation, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued
Net Ionic Equations, continued
Overall ionic equation
net ionic equation

13. Writing a Net Ionic Equation
Section 1 Compounds in Aqueous Solution
Chapter 13
Writing a Net Ionic Equation

14. Dissociation, continued Net Ionic Equations, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued Net Ionic Equations, continued
Sample Problem B
Identify the precipitate that forms when aqueous solutions of lead (II) nitrate and sodium chloride are combined. Write the equation for the possible double-displacement reaction. Then write the formula equation, overall ionic equation, and net ionic equation for the reaction.

15. Dissociation, continued Net Ionic Equations, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued Net Ionic Equations, continued
Sample Problem B Solution
Given: identity of reactants: lead (II) nitrate and sodium chloride
reaction medium: aqueous solution
Unknown: a. equation for the possible double-displacement
reaction
b. identity of the precipitate
c. formula equation
d. overall ionic equation
e. net ionic equation

16. Dissociation, continued Net Ionic Equations, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued Net Ionic Equations, continued
Sample Problem B Solution, continued
Solution:
a. equation for the possible double-displacement reaction
Pb(NO3)2(aq) + 2 NaCl(aq)  PbCl2(?) + 2 NaNO3(?)
b. Table 1 reveals that zinc sulfide is not a soluble sulfide and is therefore a precipitate. Ammonium nitrate is soluble according to the table.
c. The formula equation
Pb(NO3)2(aq) + 2 NaCl(aq)  PbCl2(s) + 2 NaNO3(aq)

17. Dissociation, continued Net Ionic Equations, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Dissociation, continued Net Ionic Equations, continued
Sample Problem B Solution, continued
d. The overall ionic equation
Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2Cl-(aq) 
PbCl2(s) + 2 Na+(aq) + 2 NO3-(aq)
The sodium and chloride ions appear on both sides of the equation as spectator ions.
The net ionic equation:
Pb2+(aq) + 2Cl-(aq)  PbCl2(s)

18. Practice Problems
Page #1-4
Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined? If so, write the net ionic equation for the reaction.
Will a precipitate form if solutions of potassium nitrate and magnesium sulfate are combined? If so, write the net ionic equation
Will a precipitate form if solutions of barium chloride and sodium sulfate are combined? If so, identify the spectator ions and write the net ionic equation.
Write the net ionic equation for the precipitation of nickel (II) sulfide

19. Section 1 Compounds in Aqueous Solution
Chapter 13
Ionization
Ions are formed from solute molecules by the action of the solvent in a process called ionization.
When a molecular compound dissolves and ionizes in a polar solvent, ions are formed where none existed in the undissolved compound.
Hydrogen chloride, HCl, is a molecular compound that ionizes in aqueous solution.
HCl contains a highly polar bond.

20. Chapter 13 Ionization, continued The Hydronium Ion
Section 1 Compounds in Aqueous Solution
Chapter 13
Ionization, continued
The Hydronium Ion
Some molecular compounds ionize in an aqueous solution to release H+.
The H+ ion attracts other molecules or ions so strongly that it does not normally exist alone.
The H3O+ ion is known as the hydronium ion.

21. Strong and Weak Electrolytes
Section 1 Compounds in Aqueous Solution
Chapter 13
Strong and Weak Electrolytes
Electrolytes are substances that yield ions and conduct an electric current in solution.
The strength with which substances conduct an electric current is related to their ability to form ions in solution.
Strong and weak electrolytes differ in the degree of ionization or dissociation.

22. Models for Strong and Weak Electrolytes and Nonelectrolytes
Section 1 Compounds in Aqueous Solution
Chapter 13
Models for Strong and Weak Electrolytes and Nonelectrolytes

23. Strong and Weak Electrolytes, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Strong and Weak Electrolytes, continued
Strong Electrolytes
A strong electrolyte is any compound whose dilute aqueous solutions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions.
To whatever extent they dissolve in water, they yield only ions.
HCl, HBr, HI
All soluble ionic compounds
Example:

24. [HF] >> [H+] and [F–]
Section 1 Compounds in Aqueous Solution
Chapter 13
Strong and Weak Electrolytes, continued
Weak Electrolytes
A weak electrolyte is any compound whose dilute aqueous solutions conduct electricity poorly; this is due to the presence of a small amount of the dissolved compound in the form of ions (only ~10% ionization.
Some molecular compounds form aqueous solutions that contain not only dissolved ions but also some dissolved molecules that are not ionized.
[HF] >> [H+] and [F–]

25. Practice Problems
The following solutions are combined in a beaker: NaCl, Na3PO4, and Ba(NO3)2. a) Will a precipitate form? If so, provide the name and the formula of the precipitate. List all spectator ions in the system.
Acetic acid, CH3CO2H,is a week electrolyte. Write an equation to represent its ionization in water. Include the hydronium ion, H3O+(aq)
Hydroiodic acid, HI(aq) is a strong acid and creates a strong electrolytic solution when mixed with water. Write an equation to represent its ionization in water. Include the hydronium ion, H3O+(aq)

26. End of Chapter 13-1 Show