1. Chapter 4 – Reactions in Aqueous Solutions

2. Aqueous Solutions
Solution – homogenous mixture of two or more substances. Solute - substance that is being dissolved.(present in smaller amounts) Solvent – usually water ( present in larger amounts) Electrolyte – substance that can dissolve in water & can conduct electricity. Non electrolyte – substance that may dissolve in water & does not conduct electricity.

3. Electrolytes
Strong Electrolytes – conduct electricity very efficiently (bulb shines brightly). 100% dissociation in water. Ex: Strong acids & bases Weak Electrolytes – conduct only a small amount of electricity (bulb glows dimly). Not completely dissociated in water. Ex: acetic acid Non electrolytes – no current flows (bulb remains unlit). Dissolves but does not produce any ions.

4. Precipitation Reactions or double displacement reactions
A double displacement reaction in which a precipitate forms (insoluble substance) and separates from the solution. Soluble – solid dissolves in solution; (aq) is used in reaction equation. Insoluble – solid does not dissolve in solution; (s) is used in reaction equation.

5. Solubility Rules
Ionic Compounds- Solubility Rules

6. Soluble/ Insoluble
NiCl2
Ag2S
Cs3PO4
(NH4)2SO4
PbCl2
Ba(OH)2

7. Double-Replacement Reactions
In a double-replacement reaction, two ionic compounds in aqueous solution switch anions and produce an insoluble substance or precipitate.
Ex:AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)

8. Double-Replacement Reactions
Reaction between barium chloride & potassium chromate:
Molecular Equation:
BaCl2(aq) + K2CrO4(aq) → BaCrO4(s) + 2 KCl(aq)
Ionic Equation:
Ba2+(aq)+2Cl-(aq)+2K+(aq)+CrO42-(aq)BaSO4(s)+2K+(aq)+2Cl-(aq)
Net Ionic Equation:
Ba2+(aq)+ CrO42-(aq)BaSO4(s)

9. Double-Replacement Reactions practice
Write molecular equation, ionic equation & net ionic equation for the reaction of sodium chloride with lithium nitrate.

10. Double-Replacement Reactions practice
Write molecular equation, ionic equation & net ionic equation for the reaction of hydrochloric acid & sodium carbonate.

11. Activity Series
When a metal undergoes a single replacement reaction, it displaces another metal from a compound or aqueous solution. The more active metal can displace the other metal. Activity series - metals are arranged according to its ability to undergo a reaction.

12. Activity Series of metals
Metals that are most reactive appear first in the activity series. Metals that are least reactive appear last in the activity series.

13. Activity Series Which of the following reactions will occur?
Ni(s) + Zn2+(aq) 
Pb(s) + Ag+(aq) 
Zn(s) + Ca2+(aq) 
Al(s) + Fe2+(aq) 

14. Molarity
Molarity (M) = moles of solute(n) per volume of solution in liters (VL)

15. Molarity Practice
How many mL of 1.50M KOH solution are needed to supply mol of KOH?

16. Dilution
Dilution is the procedure for preparing a less concentrated solution from a more concentrated solution. Moles of solute before dilution = moles of solute after dilution M1V1 = M2V2

17. Dilution Practice
If 200 mL of a 2.5M NaOH solution is diluted to 500 mL, what is the new concentration of NaOH?

18. Acids & Bases -Titrations
na MaVa = nbMbVb na = number of ionized acid ions nb = number of ionized base ions Ex: What volume of 0.115M HClO4 solution is required to neutralize 50 mL of M Ca(OH)2?

19. Oxidation- Reduction reactions or Redox Reactions
Reactions in which one or more electrons are transferred.
Oxidation – increase in oxidation state (loss of electrons) - reducing agent
Reduction – decrease in oxidation state (gain of electrons) - oxidizing agent

20. Rules for Assigning Oxidation States
Oxidation state of an atom of a free element = 0
Ex: Na, K, Pb, O2, P4 = 0
Oxidation state of monatomic ion = charge of the ion
Ex: Na+, Na = O2-, O = -2
Oxygen = -2 in covalent compounds (except in peroxides, H2O2 and O22-, where it = -1)
Hydrogen = +1 in covalent compounds (except when bonded to metals as a binary compound, where the oxidation number = -1)
Group IA metals are +1, Group IIA metals are +2, and Fluorine is always -1
Sum of oxidation states = 0 in compounds
Sum of oxidation states = charge of the ion in ions

21. Find the oxidation number for each of the elements in each of the following compounds:
K2CO3
HCO3-
MnO4 2-
NalO3
K2Cr2O7; K = +1; Cr = +6; O = -2
CO32-; C = +4; O = -2
MnO2; Mn = +4; O = -2
PCl5; P = +5; Cl = -1
SF4; S = +4; F = -1

22. Oxidation Reduction Reactions
Zn (s) + CuSO4 (aq)  ZnSO4 (aq) + Cu (s) Oxidized/Reducing Agent  Zn Reduced/Oxidizing Agent  Cu 2Mg (s) + O2 (g)  2MgO (s) Oxidized/Reducing Agent  Mg Reduced/Oxidizing Agent  O2