1. Chemical Reactions and Solution Stoichiometry
Chapter 4
Chemical Reactions and Solution Stoichiometry

2. Water: The Common Solvent
Essential for most biological reactions
Polar covalent molecule
Partial charges create poles (dipole moments)
Polarity gives water the ability to dissolve compounds

3. Water Hydration of a Solute
Hydration-the interaction between solute particles and water molecules

4. Water Hydration of a Solute
When ions dissolve, they break up into individual ions
NH4NO3(s) NH4+(aq) + NO3-(aq)
HOWEVER, solubility varies greatly among ionic compounds
Solubility depends on relative attractions of ions for each other (to be covered in CHpt 11)
Take home message:
An ionic solid dissolves into dispersed ions in water upon hydration

5. Non-ionic solubility
Non ionic compounds can be soluble if they have a polar bond.
Examples:
ethanol C2H5OH
Methanol CH3OH
Acetone (CH3)2CO
Rule of Thumb
Polar molecules are soluble, “like dissolves like”

6. Non soluble Compounds/ions
Carbonate (CO32- )
Phosphate (PO43- )
ETC………………………………………………………………………………………………………………………………………………
Non-polar molecules (animal fat)

7. Characterization of Solutions
Electrical Conductivity
Strong electrolytes: dissolve and completely ionize in water
Strong conductors of electricity
Soluble Salts, Strong Acids, Strong Bases
Weak electrolytes: small degree of ionization
Weak conductors of electricity (but STILL CONDUCT!!)
Weak acids (Acetic Acid), weak bases (NH3)
Non-electrolytes: dissolve but no ionization
Ie; Sucrose (C12H22O11), Ethanol (C2H5OH)

8. Composition of Solutions
Molarity=
Moles of solute
liters of solution
What is the molarity of a 0.30 liter solution containing 0.50 moles of NaCl?
How many liters of solution are needed to make a 1.66 M solution containing 2.11 moles of KMnO4?

9. Composition of Solutions
What is the molarity in 650. ml of solution containing 63 grams of NaCl?
How many grams of Ca(OH)2 are needed to produce 500. ml of 1.66 M Ca(OH)2 solution?
What volume of a 0.88 M solution can be made using 130. grams of FeCl2?

10. Composition of Solutions
Dilutions
Moles solute before = moles after
M1V1=M2V2
How do you prepare a 250.-ml of a 2.35 M HF dilution from a 15.0 M stock solution?
If 65.5 ml of HCl stock solution is used to make 450.-ml of a M HCl dilution, what is the molarity of the stock solution?

11. Tonight’s Homework Worksheet I just handed you 
Pg 180-#’s 15,16,21-25
Read Chapter 4, Sections 1-5 (20 pgs)
DO IT OR YOU WILL BE BEHIND TOMORROW!!!!

12. Types of Solutions FOR EXAMPLE Pb(NO3)2(aq) + KCl(aq)
Precipitation Reactions- aqueous solutions form an insoluble precipitate (duh…)
Involves using solubility rules (pg 150 Table 4.1) to determine the solid precipitate.
FOR EXAMPLE
Pb(NO3)2(aq) + KCl(aq)

13. Pb(NO3)2(aq) + KCl(aq)  PbCl2(s) + KNO3(aq)
We know that:
Most nitrates salts are soluble.
Most Group I salts are soluble.
Most Chloride salts are soluble with the exception of Pb+2 and others.
Therefore, we determine the products to be:
Pb(NO3)2(aq) + KCl(aq)  PbCl2(s) + KNO3(aq)

14. Describing reactions/ Writing equations
Molecular Equation:
Pb(NO3)2(aq) + 2KCl(aq)  PbCl2(s) KNO3(aq)
Complete ionic Equation
Pb+(aq) + 2NO3-(aq) + 2K+(aq) + 2Cl-(aq)  Pb+2(s) + 2Cl-(s) + 2K+(aq) + 2NO3-(aq)
Net Ionic Equation (get rid of the spectator ions)
Spectator ions: present in the aqueous solution before and after reaction. In this case, K+and NO3-
Indicate ions that form precipitate.
Pb+(aq) + 2Cl-(aq)  PbCl2(s)

15. Solution Stoichiometry
Steps to solving Solution Stoichiometry
1. Identify Species, determine reaction
2. Write balanced net ionic equation
3. Calculate moles of reactants
4. Determine limiting reactant
5. Calculate moles of product
6. Convert to proper unit, sig figs, etc…

16. Step 1: NaCl(s) + AgNO3(aq)  AgCl(s) + NaNO3(aq)
Calculate the mass of solid NaCl that must be added to 1.5L of a .100M AgNO3 solution to precipitate all the Ag+ ions in the form of AgCl
Step 1: NaCl(s) + AgNO3(aq)  AgCl(s) + NaNO3(aq)
Step 2: Ag+(aq) + Cl-(aq)  AgCl(s)
Step 3: 1.5L x .1M Ag+ = ?
Step 4?
Step 5?
Step 6?

17. 1Ag+(aq) + 1Cl-(aq)  1AgCl(s)
Calculate the mass of solid NaCl that must be added to 1.5L of a .100M AgNO3 solution to precipitate all the Ag+ ions in the form of AgCl
1Ag+(aq) + 1Cl-(aq)  1AgCl(s)
Step 3: Using a 1:1 mole ratio from the balanced equation
1.5L x .1M Ag+ = .150 mol Ag+
.150 mol NaCl x (58.45g NaCl/1mol)= 8.77g NaCl
Step 4?
Step 5?
Step 6?

18. More homework 
Pg 181 #’s 29-36, 39-44

19. Acid-Base Reactions
Acids-produce H+ ions when dissolved in water. A proton donor.
Bases-produce OH- ions when dissolved in water. A proton acceptor
H+(aq) + OH-(aq)  H20(l)

20. Solution Stoichiometry for Acid-Base Reactions
Steps to solving Solution Stoichiometry
1. Identify Species, determine reaction
2. Write balanced net ionic equation
3. Calculate moles of reactants
4. Determine limiting reactant
5. Calculate moles of product
6. Convert to proper unit, sig figs, etc…

21. Solution Stoichiometry for Acid-Base Reactions
FOR EXAMPLE
What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
In reality, all you are trying to do is match the moles of hydroxide ions with moles of hydrogen ions.
1. Identify Species, determine reaction
2. Write balanced net ionic equation
Involves using solubility rules (pg 150 Table 4.1) to determine a solid precipitate and spectator ions

22. 1. Identify Species, determine reaction, mole ratio
What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
1. Identify Species, determine reaction, mole ratio
HCl(aq) + NaOH(aq)  NaCl(s) + H20(l)
Mole ratio of 1:1:1:1
Remember your solubility rules,
Remember that you cannot dissolve water in water, so water is always in the “liquid” state of matter. (Sounds stupid but you would be surprised).

23. 2. Write balanced net ionic equation
What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
2. Write balanced net ionic equation
Involves using solubility rules (pg 150 Table 4.1) to determine spectator ions.
Complete ionic equation:
H+(aq) + Cl-(aq) + Na+ (aq) + OH- (aq)  H2O(l) + Na+(aq) + Cl-(aq)
Na+ and Cl- are soluble, so they exist as ions in solution. Therefore, the actual reaction does not take place. They are spectator ions.
H+(aq) + OH-(aq)  H2O(l)

24. What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
3. Calculate moles of reactants (don’t forget your mole ratios in this step!)
M = n / V
.350M HCL = n / 0.025L
n= moles  account for sig figs 8.75 x 10-3 moles (preferred by AP graders)

25. What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
4. Determine limiting reactant
We are adding a reactant, therefore we do not care about a limiting reactant. But in reality it is a 1:1 mole ratio so there isn’t one.

26. What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
5. Calculate moles of reactant needed (HCl solution)
We have a 1:1 mole ratio of hydrogen ions to hydroxide ions.
Moles H+ = Moles OH- in order to reach neutralization point
Therefore, we need 8.75 x mol H+ (present in HCl)

27. What Volume of a .100M HCl solution is needed to neutralize 25.0 mL of .350M NaOH?
6. Convert to proper unit, sig figs, etc…
The question asks us for the volume of .1M HCl
So:
M = n / V  V = n / M
VHCl= x 10-3 mol H+
.100 mol H+ / L
VHCl= 8.75 x 10-2

28. More homework…
Pg 182 #’s 45-50

29. Acid-Base titrations Key vocabulary
Volumetric Analysis-technique for determining the amount of substance through titration
Titration-delivery of a measured volume of a known solution into a substance of unknown concentration
Titrant
Analyte
Equivalence point-the point at which enough titrant has been added to react exactly with the analyte
Indicator-a substance that changes color at or near the equivalence point
Endpoint-point actual point where the indicator changes color

30. Acid-Base titrations Requirements for sucessful titrations
1. exact reaction between titrant and analyte must be known
2. Equivalence point must be marked accurately (.15 mL of titrant added, etc…)
3. Volume of titrant required to reach equivalence point must be known accurately (to calculate percent error)

31. Acid-Base Titrations
Basically, a titration is a neutralization reaction, so we follow the same rules as before.
The goal is to react an equal hydrogen ions to react with hydroxide ions.

32. Acid-Base Titrations
For Example: A student dissolves g KHC8H4O4 (KHP) in distilled H20, adds Phenolphthaleine as an indicator, and titrates with NaOH. It was found that 41.20mL of NaOH is required to react with the g KHP. What is the concentration of the sodium hydroxide?

33. 1. Identify Species, determine reaction, mole ratios
A student dissolves g KHC8H4O4 (KHP) in distilled H20, adds Phenolphthaleine as an indicator, and titrates with NaOH. It was found that 41.20mL of NaOH is required to react with the g KHP. What is the concentration of the sodium hydroxide?
1. Identify Species, determine reaction, mole ratios
KHC8H4O4(aq) + NaOH(aq)  KOH + NaHC8H4O4(aq)
2. Write balanced net ionic equation
K+ + HC8H4O4-(aq) + Na+ + OH-(aq)  K+ + OH- + NaHC8H4O4(aq)

34. Oxidation-Reduction Reactions
Redox reaction-one or more electrons are transferred
Oxidation state (number)-the imaginary charges the atoms would have if the shared electrons were divided equally between identical atoms bonded to each other (huh?)

35. Rules for assigning Oxidation States
Pg 167, Table 4.2 of your textbook
Memorize it…
More importantly, memorize exceptions to the norm

36. Oxidation number Practice
Assign Oxidation states to all atoms in the following
CO2
SF6
NO3-
CH3-
H2O2
H2O
START WITH FIRST DRAWING THE MOLECULE, oxidation states do not have to be whole numbers (for some atoms)
KMnO4
NiO2
K4Fe(CN)6
N2H4
FeO4
Na2C2O4

37. Oxidation-Reduction Reactions
Oxidation-increase in oxidation state (loss of electron). Ie, going from -1 to +1
Reduction- decrease in oxidation state (gain of an electron). Ie, going from +1 to -1
Oxidizing agent-the electron acceptor
Reducing agent-electron donor

38. Identification of Oxidizers, reducers
2Al (s) + 3I2  2AlI3
Step 1: balance equation, assign oxidation states to reactants
Step 2: assign oxidation states to products
Step 3: Identify who gained electrons (reducing agent
Step 4: Identify who lost electrons (oxidizing agent)
This was an easy problem

39. Identification of Oxidizers, reducers
Identify the oxidizing and reducing agents
PbO(s) + CO2(g)  Pb(s) + CO2(g)
CH4(g) + O2(g)  CO2(g) + H2O(l)
Cr2O72-(aq) + HCl  ZnCl2(aq) + H2(g)

40. Homework 
Pg , #s 57-62