1. Chapter 4 Acid/base, precipitaton, redox
Reactions in Solution
Chapter 4
Acid/base, precipitaton, redox

2. Water
Is an angular or bent molecule therefore polar
Types of solvation
Hydration
Dissociation
Dissociation equations
NaCl(s) → Na+ (aq) + Cl-(aq)
BaCl2(s)→ Ba2+ (aq) + 2Cl-(aq)

3. Electrolytes – Strong electrolytes Weak Electrolytes Salts
Increase [ ] =
Strong Acids
HX + H2O→ H3O+ (aq) + X- (aq)
Strong bases
MOH (s) → M+ (aq) + OH- (aq)
Weak Electrolytes
weak acids
weak bases

4. Non-electrolytes-
Molecular substances that are not acids

5. Solution Concentrations

6. Most Common unit of concentration is Molarity (M)
Example
What is the molarity of a solution made by dissolving 38.6g calcium chloride in enough water to make 475.0mL of solution?

7. Ex. 2
What volume ofj 3.67M aluminum chloride contains 2.5g of solute?
Ex. 3
How many moles of ammonium ions are contained in 35.6mL of 0.639M ammonium sulfide?

8. Preparing Solutions to a specific concentration
For solids-
Use desired molarity to convert desired volume of solution into mass of solute
For stock solutions-
MSVS = MNVN
solve for the volume of stock solution needed and dilute with water to the total desired volume

10. Ex. How would you prepare 500.mL of 0.3750N sodium chloride from:
Solid sodium chloride?
A 5.00M stock solution?

11. Precipitation Reactions

12. Precipitate:
Solubility Rules:

13. Molecular Equation:
Total Ionic Equation:
Net Ionic Equation:

14. Predict the products for the following reactions
Predict the products for the following reactions. Write the net ionic equation.
Magnesium chloride + lead (II) nitrate
Barium chlorate + sodium sulfate
Sodium hydroxide _ copper(II) chloride

15. You do these Iron (II) sufate + potassium chloride Al(NO3)3 + Ba(OH)2
Calcium chloride + sodium sulfate
Lead (II) nitrate + sodium chloride
K2S + Ni(NO3)2

16. Precipitation stoichiometry
Identify the species present in combined solution
Write a balanced NIE
Calculate moles of reactants
Determine the LR
Calculate moles of product(s) as required
Convert moles to other units as necessary

17. Stoichiometry of Precipitation Reactions
What mass of precipitate forms when mL of 3.75 M AgNO3 reacts with mL of 4.50 M NaCl?

18. What volume of 3.38 M CuSO4 is needed to completely precipitate all of the hydroxide ions in 45.6 mL of 4.39 M NaOH?

19. 100.0 mL of 0.32 M Pb(NO3)2 and 100.0 mL of 0.41 M Na2CrO4
Consider a mixture of:
100.0 mL of 0.32 M Pb(NO3)2 and mL of 0.41 M Na2CrO4
a) What mass of precipitate can be formed?
b) What is the molar concentration of all ions remaining in solution?

20. A mixture is prepared by adding 25. 0 mL of 0
A mixture is prepared by adding mL of M aluminum chloride to 75.0 mL of M potassium hydroxide. What is the concentration of all ions remaining in solution?

21. Determine the molarity of all ions in solution for the example below: mL mL M M NaOH (aq) + CuSO4 (aq) 

22. Determine the molarity of all ions in solution for the example below: 75.0 mL 35.0 mL 0.210M M CaCl2 (aq) + AgNO3 (aq) 

23. Acid Base Reactions

24. Acid base rxns are Proton transfer rxns
Arrhenius
Acids: produce _______________in aqueous sln
Bases: produce ____________in aqueous sln
Bronsted-Lowry
Acids: proton ____________
Bases: proton ____________
Acid base rxns are Proton transfer rxns
Redox rxns are electron transfer rxns

25. Lewis Acids and bases “Have pair will share”
Bases are electron pair donors
Acids are electron pair acceptors
Usually ammonia with a trigonal compound of Boron
Group 5A with BX3

26. Conjugate Acid-Base Pairs
Conjugate acids : species formed after base accepts H+
Ex: Base: NH3, F-, H2O
CA:
Conjugate base: species left once acid donate H+
Ex: Acid: HCl , HC2H3O2 , H2S , HS-
CB:

27. Amphoteric – substances that can act as an acid or a base
Acid: have hydrogen to donate
Bases: are – charged so it can accept a H+
Ex:
HS- HSO4- H2O H2PO4-

28. Stoichiometry of Acid-Base Reactions
Definitions:
volumetric analysis
Titration
Titrant
Analyte
equivalence point
Indicator
end point
"Standardizing the solution"

29. Examples:
What volume of M Ba(OH)2 will react completely with 25.0 mL of M HCl?

30. A 50.0 mL sample of an ammonia solution is analyzed by titration with HCl. The titration required mL of M HCl to reach the endpoint. What was the concentration of the ammonia solution?

31. Suppose that 5. 00 g of solid iron (III) oxide is added to 20
Suppose that 5.00 g of solid iron (III) oxide is added to 20.0 mL of M HCl.
a) What is the concentration of Fe3+ when all of the HCl has reacted?
b) What mass of Fe2O3 will not be reacted?

32. A mixture is prepared by adding 50. 0 mL of 0. 200 M HCl to 45
A mixture is prepared by adding 50.0 mL of M HCl to 45.0 mL of M KOH. Is the resulting solution acidic, basic, or neutral?