chapter 8 reactions in aqueous solution. will a reaction occur? driving forces in a chemical...
TRANSCRIPT
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Chapter 8
Reactions in Aqueous Solution
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Will a reaction Occur?
Driving Forces in a Chemical ReactionFormation of a solidFormation of waterFormation of a gasTransfer of electrons
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Types of Reactions Double Replacement Reactions
1. Precipitation Reactions
2. Acid and Base Reactions
Red-ox Reactions 3. Single Replacement Reactions
4. Synthesis Reactions
5. Decomposition Reactions
6. Combustion Reactions
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Double Replacement Reactions
1 – Precipitation Reactions
2 – Acid and Base Reactions
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Double Replacement Reactions – Reactions involving two compounds in which two elements switch places
General Form:
AB + CD → AD + CB
Double Replacement
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Solid Formation: Precipitation Reactions
(#1) Precipitation Reaction – a reaction that produces a precipitate
K2CrO4 (aq) + Ba(NO3)2 (aq) →
BaCrO4 (s) + 2 KNO3 (aq)
In order to know what will form, you need to know what is in solution!
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Solid Formation
In solution, most compounds break down into their ions Ba(NO3)2 (aq) → Ba2+
(aq) + 2 NO3
1- (aq)
Strong Electrolyte – completely dissociates into ions in solution (dissolving.mov)
The reaction is best demonstrated by:
2 K1+ (aq) + CrO42-
(aq) + Ba2+(aq) + 2 (NO3)1- (aq) → BaCrO4 (s) + 2 K1+ (aq) + 2 NO3
1- (aq)
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Solid Formation - Solubility Rules
Soluble solid – a solid that dissolves in water Insoluble solid – a solid that does not dissolve
in water Slightly soluble solid – a small amount of the
solid dissolves in water
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Solid Formation - Solubility Rules
Soluble –NO3
- salts
Na+, K+, NH4+ salts
Cl-, Br-, I- salts, but not when with Ag+, Hg2
2+, and Pb2+
SO42- salts, but not when with Ba2+ , Pb2+,
and Ca2+
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Solid Formation - Solubility Rules
InsolubleS2-
CO32-
PO43-
OH-, but not when with Na+, K+, Ca2+
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Visualizing Solubility
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Describing reactions in Aqueous Solutions
Molecular Equation – Represents all molecules involved in a reaction
Complete Ionic Equation – represents all of the ions in the reacting solution
Net Ionic Equation – shows only the ions directly involved in the reaction, spectator ions are not included
Spectator Ions – ions that are listed in the complete ionic equation, but not in the net ionic equation. They are not involved in the reaction.
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Describing reactions in Aqueous Solutions
Molecular Equation Pb(NO3)2 (aq) + Na2SO4 (aq) → PbSO4 (s) + 2NaNO3 (aq)
Net Ionic Equation Pb2+ (aq) + SO4
2-(aq) → PbSO4 (s)
Complete Ionic Equation Pb2+ (aq) + 2(NO3)- (aq) + 2Na1+ (aq) + SO4
2-(aq) → PbSO4 (s) + 2Na+ (aq) + 2NO3
- (aq)
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Describing reactions in Aqueous Solutions
Write the balanced molecular, ionic, and net ionic equations: Aqueous sodium chloride is added to aqueous silver
nitrate to form solid silver chloride plus sodium nitrate
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Formation of Water: (#2) Acids & Bases
Acid – “acidus” or sour – a substance that produces H+ ions (protons) when it is dissolved in waterStrong acid – completely dissociates in waterHCl(aq) → H1+ (aq) + Cl1- (aq)
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Base – “alkalis” slippery in feel and sour in taste – a substance that produces hydroxide (OH) ions in solutionStrong base – completely dissociates in waterNaOH(aq) → Na1+ (aq) + OH1- (aq)
Formation of Water: (#2) Acids & Bases
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Formation of Water: Acids & Bases
When acids and bases react, they neutralize each other
Neutralization – When a strong acid and strong base react to form water and an aqueous salt
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Acids & Bases
Write the molecular, Complete ionic, and net ionic equation for the reaction of nitric acid and potassium hydroxide
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Arrhenius ModelAcids – anything that produces H1+Bases – anything that produces OH1-Strong – Completely dissociates
Bronsted-LowreyAcids – Proton DonorBases – Proton AcceptorWeak – Slightly Soluble, slight dissociation
Acids & Bases
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Acid + Base → Conjugate Acid + Conjugate Base
H2SO4 + NaOH → H2O + Na2SO4
To find the conjugate acid – follow the hydrogen
To find the conjugate base - follow the anion from the acid
Acids & Bases
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Concentration – How much material is dissolved in your solution Concentrated – much material is dissolved Dilute – little material is dissolved
Molarity – Unit of Concentration in Chemistry The number of MOLES of material per LITER of
solution Unit = M M = moles / L Example: 8M HCl = an 8 Molar solution of
Hydrochloric Acid, 8 moles of HCl are dissolved in every liter of the solution
Acids & Bases
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Titration – measuring the exact amount of an acid that reacts with an exact amount of a base. If you know the concentration of one of the solutions,
it can be used to calculate the concentration of the other
Equivalence point – the point of neutralization, the amount of acid and base are equal in solution
Standard Solutions – solutions of known concentration
Acids & Bases
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Acids & Bases
Burette – the tool used to dispense an exact amount of a standard solution in a titration
Indicators – substances that change from clear to a color at a specific pH
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Acids & Bases
Titration Curve – graphing pH of solution versus volume of base added
M1V1 = M2V2
Used in Acid/Base Used in Dilution
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Example Problem: A 100.0mL solution of 0.5M HCl(aq) is titrated with 0.10M
NaOH. What volume of NaOH do you need to reach equivalence?
M 1 V 1 = M 2 V 2
MHClVHCl = MNaOHVNaOH
(100.0mL HCl)(0.50M HCl) = (X mL NaOH)(0.10M NaOH)
X = 500.0mL NaOH
Acids & Bases
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pH – measure of acid strength, equal to the molarity of the H+ ions in solution 1-14 scale 1 = strongest acid 14 = strongest base 7 = neutral Logarithmic Scale, a change of 1 pH is different in
concentration by a factor of 10! pOH – measure of base strength, equal to the
molarity of the OH- ions in solution
Acids & Bases
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Acids & Bases
Useful pH Equations: pH = -Log[H+] pOH = -Log[OH-] 14 = pH + pOH [H+] = 10(-pH)
[OH-] = 10(-pOH)
[OH-] [H+] = 1 x 10-14
[ ] = symbol of Molarity
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Oxidation – Reduction Reactions
3 – Single Replacement Reactions4 – Synthesis5 – Decomposition6 – Combustion Reactions
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Oxidation - Reduction
Oxidation/Reduction Reaction – a reaction that involves the transfer of electrons Usually between a metal and nonmetal to form an
ionic compound Involves 2 half reactions
Oxidation – loosing electrons Reduction – gaining electrons Potassium.mov zinc&iodine.mov
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Oxidation - Reduction
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2 Mg (s)+O2 (g) → 2 MgO (s)
OxidationMg → Mg 2+ + 2e-
ReductionO2 + 4e- → 2O2-
Oxidation - Reduction
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Single Replacement Reaction – Single element combines with a compound, replacing one of the members of the compound.
A + BC → AC + B
Oxidation – Reduction: (#3) Single Replacement
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Activity / Electromotive Series
Metals Nonmetals lithium fluorine potassium chlorine calcium bromine sodium iodine magnesium aluminum zinc chromium iron nickel tin lead hydrogen copper silver mercury platinum gold
Used to predict if a red-ox reaction will occur
Metals replace metals. Nonmetals replace
nonmetals. The replacing
substance must be more active (higher on the list) than the substance it replaces for a reaction to occur.
Oxidation – Reduction
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Predict if a chemical reaction will occur in the following redox reactions:
iron + copper (II) sufate
chlorine + potassium bromide
copper + zinc chloride
Oxidation - Reduction
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Oxidation – Reduction: (#4)Synthesis + (#5)Decomposition
Synthesis – Elements combining to make a compound A + B → AB Synthesis.MOV
Decomposition – Compound separating into its constituent elements AB → A + B Decomposition.MOV
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Combustion Reactions – any reaction that consumes carbon and oxygen to produce carbon dioxide and water
• General Form: CxHy + O2 → CO2 + H2O
• Example: CH4 + 2O2 → CO2 + 2H2O
Formation of a Gas: Combustion Reactions
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Top 4 ReactionsSingle ReplacementDouble DisplacementSynthesisDecomposition
Four Types.movsugar_potassiumchlorate.mov
Other Ways to Classify Reactions
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Review – Types of Reactions and Driving Forces
Double Displacement AB + CD → AD + CB Acid Base – Formation of water Multiple - Formation of gas Precipitation - Formation of a solid
Oxidation-Reduction – Driving force for all is transfer of electrons Single Replacement A + BC → AC + B Synthesis A + B → AB Decomposition AB → A + B Combustion CxHy + O2 → CO2 + H2O
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