Download General Chemistry I 2302101 Dr Rick Attrill Office MHMK 1405/5

Reactions in Aqueous Solutions
• General Properties of Aqueous solutions
General Chemistry I
• Precipitation Reactions
• Acid‐Base Reactions
2302101
• Oxidation‐Reduction Reactions
• Concentration of Solutions
Dr Rick Attrill
Office MHMK 1405/5
• Gravimetric Analysis
• Acid‐Base Titrations
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A solution is a homogenous mixture of 2 or more
substances
An electrolyte is a substance that, when dissolved in
water, results in a solution that can conduct electricity.
The solute is(are) the substance(s) present in the
smaller amount(s)
A nonelectrolyte is a substance that, when dissolved,
results in a solution that does not conduct electricity.
The solvent is the substance present in the larger
amount
Solution
Solvent
Solute
Soft drink (l)
H2O
Sugar, CO2
Air (g)
N2
O2, Ar, CH4
Soft Solder (s)
Pb
Sn
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nonelectrolyte
weak electrolyte
strong electrolyte
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Conduct electricity in solution?
Hydration is the process in which an ion is surrounded
by water molecules arranged in a specific manner.
Cations (+) and Anions (-)
Strong Electrolyte – 100% dissociation
NaCl (s)
H 2O
Na+ (aq) + Cl- (aq)
Weak Electrolyte – not completely dissociated

CH3COO- (aq) + H+ (aq)
CH3COOH

H2O
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Nonelectrolyte does not conduct electricity?
Precipitation Reactions
No cations (+) and anions (-) in solution
Precipitate – insoluble solid that separates from solution
C6H12O6 (s)
H 2O
precipitate
C6H12O6 (aq)
Strong Electrolyte Weak Electrolyte
Nonelectrolyte
HCl
CH3COOH
(NH2)2CO
HNO3
HF
CH3OH
HClO4
HNO2
C2H5OH
NaOH
H2O
C12H22O11
Pb(NO3)2 (aq) + 2NaI (aq)
PbI2 (s) + 2NaNO3 (aq)
molecular equation
Pb2+ + 2NO3- + 2Na+ + 2I-
PbI2 (s) + 2Na+ + 2NO3-
ionic equation
Pb2+ + 2IPbI2
Ionic Compounds
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PbI2 (s)
net ionic equation
Na+
and NO3- are spectator ions
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Writing Net Ionic Equations
1. Write the balanced molecular equation.
Solubility Rules for Common Ionic Compounds
In water at 250C
2. Write the ionic equation showing the strong electrolytes
Soluble Compounds
3. Determine precipitate from solubility rules
Compounds containing alkali
metal ions and NH4+
4. Cancel the spectator ions on both sides of the ionic equation
Write the net ionic equation for the reaction of silver
nitrate with sodium chloride.
AgNO3 (aq) + NaCl (aq)
Ag+
+
NO3-
+
Na+
Ag+
+
Cl-
+
Cl-
AgCl (s) + NaNO3 (aq)
AgCl (s) +
Na+ +
AgCl (s)
NO3-
Exceptions
NO3-, HCO3-, ClO3Cl-, Br-, I-
Halides of Ag+, Hg22+, Pb2+
SO42-
Sulfates of Ag+, Ca2+, Sr2+, Ba2+,
Hg2+, Pb2+
Insoluble Compounds
Exceptions
CO32-, PO43-, CrO42-, S2-
Compounds containing alkali
metal ions and NH4+
OH-
Compounds containing alkali
metal ions and Ba2+
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Acids
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Arrhenius acid is a substance that produces H+ (H3O+) in water
Have a sour taste. Vinegar owes its taste to acetic acid. Citrus
fruits contain citric acid.
React with certain metals to produce hydrogen gas.
React with carbonates and bicarbonates to produce carbon
dioxide gas
Arrhenius base is a substance that produces OH- in water
Bases
Have a bitter taste.
Feel slippery. Many soaps contain bases.
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Monoprotic acids
A Brønsted acid is a proton donor
A Brønsted base is a proton acceptor
H+ + Cl-
HCl
Strong electrolyte, strong acid
H+ + NO3-
HNO3
Strong electrolyte, strong acid
H+ + CH3COO-
CH3COOH
Weak electrolyte, weak acid
Diprotic acids
base
acid
acid
base
H2SO4
H+ + HSO4-
Strong electrolyte, strong acid
HSO4-
H+ + SO42-
Weak electrolyte, weak acid
Triprotic acids
H3PO4
H2PO4HPO42-
A Brønsted acid must contain at least one
ionizable proton!
H+ + H2PO4H+ + HPO42H+ + PO43-
Weak electrolyte, weak acid
Weak electrolyte, weak acid
Weak electrolyte, weak acid
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Oxidation-Reduction Reactions
Neutralization Reaction
(electron transfer reactions)
acid + base
HCl (aq) + NaOH (aq)
H+ + Cl- + Na+ + OHH+ + OH-
salt + water
2Mg (s) + O2 (g)
2MgO (s)
NaCl (aq) + H2O
Na+ + Cl- + H2O
2Mg
H2O
O2 + 4e-
2Mg2+ + 4e- Oxidation half-reaction (lose e-)
2O2-
Reduction half-reaction (gain e-)
2Mg + O2 + 4e15
2Mg + O2
2Mg2+ + 2O2- + 4e2MgO
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Zn (s) + CuSO4 (aq)
Zn
ZnSO4 (aq) + Cu (s)
Zn2+ + 2e- Zn is oxidized
Cu2+ + 2e-
Zn is the reducing agent
Cu Cu2+ is reduced Cu2+ is the oxidizing agent
Copper wire reacts with silver nitrate to form silver metal.
What is the oxidizing agent in the reaction?
Cu (s) + 2AgNO3 (aq)
Cu(NO3)2 (aq) + 2Ag (s)
Cu2+ + 2e-
Cu
Ag+ + 1e-
Ag Ag+ is reduced
Ag+ is the oxidizing agent
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Oxidation number
The charge the atom would have in a molecule (or an
ionic compound) if electrons were completely transferred.
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4. The oxidation number of hydrogen is +1 except when
it is bonded to metals in binary compounds. In these
cases, its oxidation number is –1.
5. Group IA metals are +1, IIA metals are +2 and fluorine
is always –1.
1. Free elements (uncombined state) have an oxidation
number of zero.
6. The sum of the oxidation numbers of all the atoms in
a molecule or ion is equal to the charge on the
molecule or ion.
Na, Be, K, Pb, H2, O2, P4 = 0
2. In monatomic ions, the oxidation number is equal to
the charge on the ion.
HCO3Oxidation numbers of all
the elements in HCO3- ?
Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2
3. The oxidation number of oxygen is usually –2. In H2O2
and O22- it is –1.
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O = -2
H = +1
3x(-2) + 1 + ? = -1
C = +4
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Types of Oxidation-Reduction Reactions
IF7
Oxidation numbers of all
the elements in the
following ?
F = -1
Combination Reaction
A+B
7x(-1) + ? = 0
I = +7
0
0
S + O2
K2Cr2O7
NaIO3
O = -2
Na = +1 O = -2
3x(-2) + 1 + ? = 0
+4 -2
SO2
Decomposition Reaction
K = +1
C
7x(-2) + 2x(+1) + 2x(?) = 0
I = +5
C
+1 +5 -2
2KClO3
Cr = +6
A+B
+1 -1
0
2KCl + 3O2
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Types of Oxidation-Reduction Reactions
Displacement Reaction
+1
+4
0
TiCl4 + 2Mg
0
-1
Cl2 + 2KBr
M + BC
AC + B
+2
Sr + 2H2O
0
Sr(OH)2 + H2 Hydrogen Displacement
0
+2
Ti + 2MgCl2 Metal Displacement
-1
The Activity Series for Metals
Displacement Reaction
A + BC
0
22
0
2KCl + Br2
Halogen Displacement
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AC + B
M is metal
BC is acid or H2O
B is H2
Ca + 2H2O
Ca(OH)2 + H2
Pb + 2H2O
Pb(OH)2 + H2
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Types of Oxidation-Reduction Reactions
Classify the following reactions.
Disproportionation Reaction
Element is simultaneously oxidized and reduced.
+1
0
Cl2 + 2OH-
-1
Ca2+ + CO32NH3 + H+
ClO- + Cl- + H2O
Zn + 2HCl
Chlorine Chemistry
Ca + F2
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CaCO3
NH4+
ZnCl2 + H2
CaF2
Precipitation
Acid-Base
Redox (H2 Displacement)
Redox (Combination)
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Solution Stoichiometry
The concentration of a solution is the amount of solute
present in a given quantity of solvent or solution.
M = molarity =
moles of solute
liters of solution
What mass of KI is required to make 500. mL of
a 2.80 M KI solution?
M KI
volume KI
500. mL x
moles KI
1L
1000 mL
x
2.80 mol KI
1 L soln
M KI
x
grams KI
166 g KI
1 mol KI
= 232 g KI
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Dilution is the procedure for preparing a less concentrated
solution from a more concentrated solution.
How would you prepare 60.0 mL of 0.2 M
HNO3 from a stock solution of 4.00 M HNO3?
MiVi = MfVf
Mi = 4.00
Dilution
Add Solvent
Vi =
Moles of solute
before dilution (i)
=
Moles of solute
after dilution (f)
MiVi
=
MfVf
Mf = 0.200
MfVf
Mi
=
Vf = 0.06 L
Vi = ? L
0.200 x 0.06
= 0.003 L = 3 mL
4.00
3 mL of acid + 57 mL of water = 60 mL of solution
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Titrations
Gravimetric Analysis
3. Filter and dry precipitate
In a titration a solution of accurately known concentration is
added gradually added to another solution of unknown
concentration until the chemical reaction between the two
solutions is complete.
4. Weigh precipitate
Equivalence point – the point at which the reaction is complete
1. Dissolve unknown substance in water
2. React unknown with known substance to form a precipitate
5. Use chemical formula and mass of precipitate to determine
amount of unknown ion
Indicator – substance that changes color at (or near) the
equivalence point
Slowly add base
to unknown acid
UNTIL
the indicator
changes color
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What volume of a 1.420 M NaOH solution is
Required to titrate 25.00 mL of a 4.50 M H2SO4
solution?
WRITE THE CHEMICAL EQUATION!
H2SO4 + 2NaOH
M
volume acid
25.00 mL x
acid
2H2O + Na2SO4
rx
moles acid
4.50 mol H2SO4
1000 mL soln
x
coef.
M
moles base
2 mol NaOH
1 mol H2SO4
x
base
volume base
1000 ml soln
1.420 mol NaOH
= 158 mL
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