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ADVANCED CHEMISTRY—Chapter 4—Chemical Reactions and Solution Chemistry
http://www.wwnorton.com/college/chemistry/chemistry3/ch/04/studyplan.aspx
Standards:
Ch4.1: I can apply the solubility rule to solutions
Ch4.2: I can illustrate dissociation correctly with equations and particle diagrams.
Ch4.3: I can differentiate between a strong, weak and non electrolyte, and predict which type a
substance would be.
Ch4.4: I can do calculations with molarity of solutions.
Ch4.5: I can do calculations with precipitation and acid base reactions.
Ch4.6: I can apply oxidation states rules to oxidation/reduction reactions.
1) Water as a Solvent (Section 4.1).
Why can water dissolve so many solids and liquids?
A) ____________ Molecule
B) Solubility Rule: ___________ dissolves _____________
C) Hydration process. Ionization/Dissociation
Ca(NO3)2(s) 
BaCl2(S) 
2) Electrolytes. (Section 4.1 & 4.3). (Q: 4.2; 4.16; 4.18; 4.38)
What evidence of hydration do we have?
A) Strong Electrolyte
Soluble Salts—
Strong Acids(p.134)—
Strong Bases(p.134)—
B) Weak Electrolyte
Weak Acids—
Weak Bases—
C) Non Electrolyte
3) Solutions (Section 4.5) (Q: 4.10; 4.20; 4.62; 4.64; 4.72; 4.74; 4.76; 4.101)
A) Concentration—How can we count the number of dissolved particles in a solution?
1) Molarity
2) Dilutions
4) Types of Chemical Reactions
A) Precipitation Reactions (Section 4.2 & 4.6) ( Q: 4.7;4.22; 4.24; 4.26a; 4.28; 4.30; 4.80; 4.87)
What happens when solutions react to form solids?
1) Precipitate/Soluble
2) Solubility Table—p. 129
3) Molecular Equations
4) Ionic Equations
5) Net-Ionic Equations
6) Spectator Ions
7) Stoichiometry—focus on balanced equation & moles
B) Acid-Base Reactions (Section 4.3 & 4.6) (4.12; 4.32; 4.40b; 4.82; 4.84; 4.106)
What happens when an acid and base react?
1) Neutralization Reactions
2) Salt--
3) Focus on balanced equation & moles
4) Titrations
Standard Solution
Equivalence Point
End Point
C) Oxidation-Reduction Reactions (Section 4.4) (Q: 4.48; 4.50; 4.52; 4.56; 4.58)
How do we track electron movement in chemical reactions?
1) Oxidation Numbers
2) Oxidation
3) Reduction
4) Activity Series—p.144
Oxidation States/Numbers Rules
1) Oxidation state of each atom in an element ==________
ex: Na; O2; Cl2
2) Oxidation state of a monoatomic ion == _____________
Ex: Na +; O 23) In compounds, the sum of the oxidation states of all atoms== _______ .
4) In compounds, Fluorine’s oxidation state is always ______. The other halogens (Cl, Br, I) have
an oxidation state of ______, except when the other element is another halogen above it on the
periodic table or the other element is oxygen.
5) Oxygen’s oxidation state is ______. Exceptions: a) in peroxides (H2O2, Na2O2) oxygen’s
oxidation state is -1. b) in OF2; O=_______ (see rule #3).
6) Hydrogen’s oxidation state is _______ when it is bonded to nonmetals (HCl) and _____ when it is
bonded to metals (NaH).
7) Atoms from group 1 of the periodic chart have an oxidation state of _____.
8) Atoms from group 2 of the periodic chart have an oxidation state of ______.
9) IN polyatomic ions, the sum of the oxidation states of all atoms == _________.
MOLARITY PROBLEMS
1) What is the molarity of a solution made by dissolving 11.5 grams of NaOH in enough
water to make a 1.5 liter solution?
2) What volume of blood serum contains 1.0 milligram of NaCl if blood serum is 0.14 M of
NaCl?
3) Calculate the number of moles of Cl- ions in a 175 ml solution of 0.001 M ZnCl2 .
4) How would you make a 250ml solution of potassium dichromate that is 0.200 M?
5) How would you make a 375 ml 2.5 M HCl solution from a stock solution of 12.0 M HCl?
PRECIPITATION EQUATIONS
Complete the ionic and net-ionic equation for combining aqueous solutions of lead (II) nitrate and
potassium iodide.
PRECIPITATION PROBLEMS
1) Sodium sulfate and lead(II) nitrate are mixed. Find the mass of precipitate formed when
1.25 liter of 0.05 M lead (II) nitrate is mixed with 2.00 liters of 0.025 M sodium sulfate.
2) Find the mass of aluminum hydroxide produced when 50.0 ml of 0.200 M aluminum
nitrate is added to 200. ml of 0.100 M KOH. Calculate the concentration of each
ion as well.
ACID/BASE PROBLEMS
1) If we mix 28.0 ml of 0.25 M HNO3 with 26.0 ml of 0.320 M Ba(OH)2 , calculate the moles of water
formed in the reaction. Also, calculate the concentration of H + or OH - ions in excess after the
reaction is complete.
2) 25.2 ml of 3.21 M HCl is titrated with Sr(OH)2 to a phenolphthalein endpoint. The difference
between the final and initial buret reading indicates that 21.20 ml of Sr(OH)2 was added. Calculate
the concentration of Sr(OH)2.
OXIDATION/REDUCTION PROBLEMS:
Determine the oxidation states of each atom in the following compounds/ions.
CaF2
H2O
KMnO4
Cr2O7 2-
ICl5
C2H6
SO4 2-
Identify the substance begin oxidized and reduced in the following reactions:
Zn
SiCl4

ZnCl2
+ H2
+ 2 Mg 
2 MgCl2
+ Si
+ 2 HCl