Chemical Solutions and Chemical Reactions Chpt 4 questions pg 171 -179 #15, 26, 27, 31, 37, 44, 48, 56, 66ac, 72, 79, 84, 106, 126 Due Fri 9/16 • Types of rxns • Redox, e - transfer • Net ionic equations
Jan 28, 2016
Chemical Solutions and Chemical Reactions
Chpt 4 questions pg 171 -179 #15, 26, 27, 31, 37, 44, 48, 56, 66ac, 72, 79, 84, 106, 126 Due Fri 9/16
• Types of rxns• Redox, e- transfer• Net ionic equations
Water Molecule“common solvent”
Polar
Because water is polar it can dissolve ionic compounds (full charges) and polar molecules (partial charges)
Polar Water Molecules Interact with Salt Ions
Water solvates the ions, (-) charged oxygen surrounds cations, (+) charged hydrogens surround anions pull them into solution
Ethanol Molecule and Water Molecule
Demonstrates water attraction for polar molecules, also a hydrogen from another water may be attracted to theoxygen on the ethanol molecule to help solvate it.
Electrical Conductivity of aqueous solutions
The brightness of the light is related to the number of ions in solution.Strong electrolytes are totally dissociated (many ions).Weak electrolytes are slightly dissociated (few ions).Non-electrolytes (no ions) are dissolved but not ionic.
Solubility of acetic acid - weak acid & ammonia - weak base
Both are weak electrolytes (few ions in solution)
Reaction Types
• Know 5 Types by name• Precipitate reactions (formation of solid)• Acid/base reactions - neutralization
reaction (formation of water) • Oxidation/reduction reactions (electron
transfer reactions)
Net Ionic Equation• Formula Equation (complete balanced
equation)• Complete ionic equation (break down
all strong electrolytes) – Know solubility rules– aqueous solutions– strong acids and bases
• Net ionic equation – Eliminate spectator ions from equation
Solubility Rules 1. All Na+, K+, alkali metal ions and NH4
+ compounds are soluble.
2. All NO31-, C2H3O2-, HClO3
1-, and ClO41-
compounds are soluble. 3. All Cl1-, Br1-, and I1- compounds are soluble,
except those with Ag1+, Hg22+, and Pb2+
4. All SO42- compounds are soluble, except PbSO4,
BaSO4, HgSO4, CaSO4, and AgSO4.
5. Most O2-, OH1-, PO43-, CO3
2-, and S2- compounds are insoluble, except those of Na+, K+, alkali metal ions and NH4
+.
Oxidation State rules
Oxidation-reduction Process
Concentration of Solutions
• Molarity M = moles of solute / liter of solution– Molarity of each ion
• Dilutions– Moles of solute doesn’t change just
increase volume of total solution
– M1 x V1 = M2 x V2
(new volume is larger so molarity is smaller)