chapter 7 reactions in aqueous solutions
DESCRIPTION
Chemistry B2A. Chapter 7 Reactions in Aqueous Solutions. Reactions in Aqueous Solutions. Ionic compounds. Aqueous solution : solvent is water. Reactions in Aqueous Solutions. Chemical reactions that occur in water. In our body reactions occur in the aqueous solution. Water in our body. - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 7
Reactions in Aqueous Solutions
Chemistry B2A
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Reactions in Aqueous Solutions
Ionic compounds
Aqueous solution: solvent is water
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Reactions in Aqueous Solutions
In our body reactions occur in the aqueous solution.
Chemical reactions that occur in water.
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Water in our body
1. About 60% of our body.
2. Most of the reactions occur in aqueous solution.
3. Participates in many biochemical reactions.
4. Transports reactants and products from one place in our body to another.
5. Eliminates the waste materials from cells and our body (urine).
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Why does a chemical reaction occur?
1. Formation of a solid
2. Formation of water
3. Transfer of electrons
4. Formation of a gas
Several driving forces:
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Why does a chemical reaction occur?
Several driving forces:
1. Formation of a solid
2. Formation of water
3. Transfer of electrons
4. Formation of a gas
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Formation of a solid
Precipitation reactions
Precipitate
KI + Pb(NO3)2 ?
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Ions Hydrated by H2OHydration
Ionic Compounds
When an ionic compound dissolves in water, ions are produced.
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Ionic Compounds
1. Soluble solid: it completely dissolves in water (ions are formed).
2. Slightly soluble solid: it partially dissolves in water.
3. Insoluble solid: it does not dissociate in water (almost).
Ionic compounds = Salts
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Ionic Compounds
Most chlorides (Cl-) and sulfates (SO42-) are soluble in water.
(except AgCl, PbCl2, BaSO4, CaSO4, PbSO4)
Most carbonates (CO32-), phosphates (PO4
3-), Sulfide (S2-), and hydroxides (OH-) are insoluble in water.
(except NaOH, KOH, Ba(OH)2, Ca(OH)2, and NH4OH)
All nitrates (NO3-) and acetate (CH3COO-) are soluble in water.
Most salts of Na+, K+, and NH4+ are soluble in water.
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+ -electrolyte
Na+Cl-
bulb
Electrolytes
Electrolyte: conducts an electric current.
Ionization (Dissociation)
NaCl → Na+ + Cl-
strong electrolytes: molecules dissociate completely into ions (NaCl).
weak electrolytes: molecules dissociate partially into ions (CH3COOH).
nonelectrolytes: molecules do not dissociate into ions (DI water).
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Formation of a solid
Precipitation reactions
Precipitate
KI + Pb(NO3)2 ?
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Aqueous Solution (ionic compounds)
KI(s) K+(aq) + I-(aq) Dissociation(Ionization)
aqueous solution: solvent is water
H2OKI
Pb(NO3)2
K+
Pb(NO3)2(s) Pb2+(aq) + 2NO3-(aq)
H2O
I-
Pb2+
NO3-
NO3-
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2KI(aq) + Pb(NO3)2(aq) PbI2(s) + 2KNO3(aq)
Aqueous Solution (ionic compounds)
KI Pb(NO3)2
K+
I- Pb2+
NO3-
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2K+(aq) + Pb2+(aq) + 2I-(aq) + 2NO3-(aq) PbI2(s) + 2K+(aq) + 2NO3
-(aq)
CompleteIonic equation:
Molecular equation:
2As3+(aq) + 3s2-(aq) As2S3(s)
total charge on left side = total charge on right sidebalanced equation
2KI(aq) + Pb(NO3)2(aq) PbI2(s) + 2KNO3(aq)
2K+(aq) + Pb2+(aq) + 2I-(aq) + 2NO3-(aq) PbI2(s) + 2K+(aq) + 2NO3
-(aq)
Pb2+(aq) + 2I-(aq) PbI2(s)Net ionic equation:
Spectator ions
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Why does a chemical reaction occur?
1. Formation of a solid
2. Formation of water
3. Transfer of electrons
4. Formation of a gas
Several driving forces:
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Acids and Bases
Acids: sour
Bases: bitter or salty
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Acids and Bases
NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)
Acid: produces H3O+ (H+) in water.
Base: produces OH- in water.
Arrhenius definition:
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
H3O+ (Hydronium ion): H+(aq) + H2O(l) H3O+(aq)
NaOH(s) Na+(aq) + OH-(aq)H2O
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Acids and Bases
Weak acid and base: it is partially ionized in aqueous solution.
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
Strong acid and base: it is completely ionized in aqueous solution.
HCl(aq) + H2O(l) Cl-(aq) + H3O+(aq)
NaOH(aq) + H2O(l) Na+(aq) + OH-(aq)
NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)
produces less H+ and OH-
produces more H+ and OH-
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Acid-Base Reactions
Neutralization
A strong acid and a strong base react together to produce a salt and water.
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)
Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) + Na+(aq) + Cl-(aq) + H2O(l)
H+(aq) + OH-(aq) H2O(l)
The only chemical change is the formation of water.
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Why does a chemical reaction occur?
1. Formation of a solid
2. Formation of water
3. Transfer of electrons
4. Formation of a gas
Several driving forces:
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Na → Na+ + e-
Cl + e- → Cl-
Oxidation and Reduction reactions (redox)
2Na(s) + Cl2(g) 2NaCl(s)
e-
Metal + Nonmetal : Transfer of electrons
Oxidation and Reduction reactions (redox)
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Oxidation and Reduction reactions (redox)
Zn(s) Zn2+(aq) + 2e- Zn is oxidized (reducing agent)
Cu2+(aq) + 2e- Cu(s) Cu2+ is reduced (oxidizing agent)
oxidation: it is the loss of electrons.reduction: it is the gain of electrons.
Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s) redox reaction
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Oxidation and Reduction reactions (redox)
oxidation: is the gain of oxygen / loss of hydrogen.reduction: is the loss of oxygen / gain of hydrogen.
CH4(s) + 2O2(g) CO2(g) + 2H2O(g) redox reaction
C gains O and loses His oxidized
(reducing agent)
O gains HIs reduced
(oxidizing agent)
single replacement reaction and combustion reactions redox reactions
double replacement reactions non redox
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Classification of chemical reactions
Chemical reactions
PrecipitationReactions
Oxidation-ReductionReactions
Acid-BaseReactions
CombustionsReactions
Synthesis (combination)Reactions
(Reactants are elements.)
Decomposition (Analysis)Reactions
(Products are elements.)