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Chapter 3-review. Some Electrical Properties of Aqueous Solutions. Reactions that Form Precipitates -Write molecular equation -Check solubility A. Aqueous: mixture of substance in water B. Soluble: dissolves in water IA salts, NH 4 + ,NO 3 - , C 2 H 3 O 2 - , chlorates, perchlorates )

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Chapter 3-review

Some Electrical Properties of Aqueous Solutions

  • Reactions that Form Precipitates
  • -Write molecular equation
  • -Check solubility
      • A. Aqueous: mixture of substance in water
  • B. Soluble: dissolves in water IA salts, NH4+,NO3-, C2H3O2- , chlorates, perchlorates)
  • C. Insoluble: does not dissolve in water OH-, S2-, CO3 2–, PO43– except Li+, Na+, K+, NH4+ etc)
  • D. Solubility rules of halides ad sulfates check from book- mostly soluble with exceptions!!

REVIEW CHAPTERS 4,5, 6(part)

Chapter 4

  • Single- Double displacement reactions
  • Precipitation reactions
    • Must know solubility charts
  • Gas forming reactions (H2CO3 breaks into H2O and CO2)
    • H2SO3 as produced as product breaks into H2O and SO2
  • Reactions of Acids and Bases-Forms salt and water
    • Acids produce H+ , bases produce OH- --Arrhenius Definition
    • Bronsted-Lowry Definition: AcidsH+ donor and bases H+ accepter
    • Strong and Weak acids (memorize strong acids)

This is the net ionic equation for the reaction.

  • Reactions that Form Precipitates
  • -Write molecular equation
  • -Check solubility
      • A. Aqueous: mixture of substance in water
  • B. Soluble: dissolves in water Li+, Na+, K+, NH4+,NO3-, C2H3O2-
  • C. Insoluble: does not dissolve in water (CO3 2–, PO43– except Li, Na, K, NH4 etc)
  • D. Solubility rules –Check Handout I gave in recitation
  • Write Equation in Solutions
  • Learn to write Molecular, Ionic and net ionic equation keeping in mind the solubility rules
  • gas forming reactions

Reactions Involving Oxidation and Reduction-Redox,

Single Dispalcement Reactions

  • -Oxidation involves LOSS of Electrons “OIL”
  • Reduction involves GAIN of Electrons “RIG”
  • Oxidation Number (ON) rules:


Single -displacement reaction,. Activity series in metals

Oxidizing agents get reduced in a reaction

Reducing agents get oxidized in reaction

Look up Single-Double displacement lab & quiz4 for Practice


Chapter 4

  • Stoichiometry – Simple one
  • Stoichiometry – Limiting reagent
  • % yield
  • Combustion Analysis to find empirical formula chapter 3

Specifying Solution Concentration: Molarity

A. Molarity (M) =

B. Volume of solution, not just solvent

C. Units always mol/L

D. Ion concentrations

Solution Stoichiometry

A. Balanced chemical equations give molar ratios only

B. Convert volume to moles using molarity, then use balanced chemical equation


concentrations of aluminum ion and of sulfate ion in 1.20 M aluminum sulfate?

  • Aluminum sulfate is an ionic compound, soluble in water. It is a strong electrolyte.

Dilution Equation: M1 V1 = M2 V2

Solution Stoichiometry

Mass of ppt formed (remember use molarity and volume in L to get moles)

Titrations ACID-BASE

At end point moles of H+ = moles of OH-

1:1 Stoichiometry Ma Va = Mb Vb (eg. HCl vs NaOH)

MONOprotic acid :DihydroxyBase Ma Va = 2*Mb Vb (HCl vs Ca(OH)2

DiproticAcid : 1hydroxybase 2* Ma Va = Mb Vb (H2SO4 vs NaOH)

Make up more combinations!


Chapter 5 Gases

Gas Pressure

Units Atm, Torr = mm Hg, pascal = Newton/m2, lbs/in2

P = h x density x g

Memorize 1 atm = 760Torr

Boyle’s Law: The Pressure-Volume Relationship

AT CONSTANT T, n :P is inversely proportional to V or PV = constant

P1V1 = P2V2

Charles’s Law: The Temperature-Volume Relationship

AT CONSTANT n, P: V is directly proportional to T or V/T = constant

V1/T1 = V2 /T2

Avogadro’s Law: The Mole-Volume Relationship

AT CONSTANT T, P: V is directly proportional to n or V/n = constant

V1/n1 = V2 /n2


The Combined Gas Law- When all (P,V, N, T) are varying


The Ideal Gas Law: Derived from combined gas law, nothing varying

At any condition, PV = nRT

P= pressure in atm, V= volume in liters, n = # of moles, T= temp in KELVIN

R = gas constant 0.082 Liter atm/Kelvin mole

Density d = MP/RT where M= molar mass of the gas

M = dRT/P

Gases in Reaction Stoichiometry

At STP (T=273K, P = 1Atm) 1 mole of a gas occupies 22.4L

- Use gas laws to convert into moles of reactant or product

- Use reaction stoichiometry to convert moles of A to moles of B

Mixtures of Gases: Dalton’s Law of Partial Pressures

Definition of mole fraction x

The Kinetic-Molecular Theory: Some Quantitative Aspects

The root mean square speed RMS

effusion rate inversely proportional to Square root of mass


Chapter 6 Thermochemistry

Energy Thermochemistry: Some Basic Terms

- Open system Energy and mass exchange

- Closed system Only energy wxcahge

- Isolated No exchange

In an exothermic process the system gives off heat to the surroundingsQ (system) = -ve

In an endothermic process the system absorbs heat from the surroundings (heat enters the system Q (system) = +ve

W = -PDV

Work done on the system W = +ve, volume decreases

Work done by the system Expansion W = -ve, volume increases

Internal Energy (U), State Functions, and the First Law of Thermodynamics

Keep track of sign of q and w

Increase in internal energy DU +ve

Decrease in internal energy DU -ve

Heats of Reaction and Enthalpy Change,DH

–State Function and Extensive Property (depends on mass, moles etc)

-Heat exchange in chemical reaction under constant T and P

Exothermic DH = -ve ; Endothermic = DH =+ve


Calorimetry: Measuring Quantities of Heat -IMPORTANT

Read definitions of heat capacity (cal/ºC) and Specific heat (cal/g ºC)

Specific of heat of water = 1cal/g ºC

Heat absorbed = q =

Calorimetry problems:

Heat lost by hot metal or reaction = Heat gained by Calorimeter or water

DT = -ve !!! DT = +ve !!!

Heat absorbed by calorimeter = qcalor = +ve = heat capacity X DT

  • Heat changes in change of state
  • Melting, Vaporization, sublimation, condensation, deposition
  • Heat exchange in chemical reactions
  • Hess’s Law problems
  • Standard enthalpy and DH for reaction =
  • sum of DH for products - sum of DH for reactants
  • Remember DH formation at standard state for elements in natural form =0
  • And for compounds we must form 1 mole of compounds using elements in natural state Formation of CaCO3 (s) is Ca(s) + C (gr,S) + 3/2 O2 CaCO3 (s)



10 points Bonus question!!

Part 1 Multiple Choice –Show calculations for partial/full credit

20 questions 3 POINTS EACH in Room T123 9:30am

Part 2 Math Problems in Lab

Bonus question: 10 points –HARD! Partial credit!