Aqueous solution reactions1 Aqueous-solution Reactions Classify a reaction by Homogeneous chemical...
-
Upload
amelia-hines -
Category
Documents
-
view
228 -
download
0
Transcript of Aqueous solution reactions1 Aqueous-solution Reactions Classify a reaction by Homogeneous chemical...
aqueous solution reactions 1
Aqueous-solution Reactions
Classify a reaction by
Homogeneous chemical reactions:
gas phasesolutions
aqueous-solution (common occurrence)non-aqueous-solution
Heterogeneous (more than one phase) chemical reactions:
gas / liquidgas / solidliquid / solid
Know the meaning of terms
aqueous solution reactions 2
Nature of Aqueous Solutions
Nature of compounds
molecular substances (polar, non-polar, H-bonding)non-electrolytes
ionic substances (acids, bases, salts)strong electrolytes (completely ionized in solution)week electrolytes (not completely ionized in solution)
Know your terms and species (in the solution)
aqueous solution reactions 3
Dissolving a Strong Electrolyte
See them in your imagination
aqueous solution reactions 4
aqueous solution reactions 5
Strong ElectrolytesStrong acids: HNO3, H2SO4, HCl, HClO4
Strong bases: MOH (M = Na, K, Cs, Rb etc)
Salts: All salts dissolving in water are completely ionized. The ions may react with water (to be discussed in Chem 123)
Stoichiometry & concentration relationship
NaCl (s) Na+ (aq) + Cl– (aq)
Ca(OH)2 (s) Ca+(aq) + 2 OH– (aq)
AlCl3 (s) Al3+ (aq) + 3 Cl– (aq)
(NH4)2SO4 (s) 2 NH4 + (aq) + SO42– (aq)
aqueous solution reactions 6
Concentration of Ions
A bottle labeled as 0.100 M Al2(SO4)3.
[Al3+] = _____ M (mol / L)
[SO42–] = _____ M
Assume sea water is 0.438 M NaCl, 0.0512 M MgCl2, and 0.001 M CaCl2
[Na+] = _____ M
[Mg2+] = _____ M
[Ca2+] = _____ M
[Cl–] = _____ M Know how to calculate your quantities
aqueous solution reactions 7
Precipitations
When ions form a solid that is not very soluble, a solid is formed. Such a phenomenon is called precipitation.
The formation of a precipitation is also an equilibrium phenomenon (a subject to be covered in Chem123)
Ag+ (aq) + Cl– (aq) AgCl(s)or AgCl(s) Ag+ (aq) + Cl– (aq) Ksp = [Ag+][Cl–] is a constant
the solubility product
aqueous solution reactions 8
Precipitation Reactions
Ag+ (aq) + NO3– (aq) + Cs+ (aq) + I– (aq) AgI (s) + NO3
– (aq) + Cs+ (aq)
Ag+ (aq) + I– (aq) AgI (s) (net reaction)or
Ag+ + I– AgI (s)
Heterogeneous Reactions
Spectator ions or bystander ions
Soluble ions
Alkali metals, NH4+
nitrates, ClO4-,
acetate
Mostly soluble ions
Halides, sulfates
Mostly insoluble
Silver halidesMetal sulfides, hydroxidescarbonates, phosphates
aqueous solution reactions 9
Acid-base Reactions HCl (g) H+ (aq) + Cl– (aq)
NaOH (s) Na+ (aq) + OH– (aq)
neutralization reaction: H+ (aq) + OH– (aq) H2O (l)
Explain these reactions
Mg(OH)2 (s) + 2 H+ Mg2+ (aq) + 2 H2O (l)
CaCO3 (s) + 2 H+ Ca2+ (aq) + H2O (l) + CO2 (g)
Mg(OH)2 (s) + 2 HC2H3O2 Mg2+ (aq) + 2 H2O (l) + 2 C2H3O2 – (aq)
acetic acid
aqueous solution reactions 10
Oxidation-reduction reactions
Oxidation reaction must be accompanied by reductions – redox reactions
Increasing oxidation state is oxidation (loss e–, LEO)Decreasing oxidation state is reduction (gain e–, GER)
What elements are oxidized and reduced in each reaction? Work out the oxidation state changes for them as well!
2 KClO3 2 KCl + 3 O2
Fe2O3 + 3 CO 2 Fe + 3 CO2
MnO2 + 4 H+ + 2 Cl– Mn2+ + 2 H2O + Cl2
aqueous solution reactions 11
Review Oxidation StatesOxidation states is an assigned number. Formal charge concept may be used to assign oxidation states.
Work out the oxidation states of all elements in these species:
NH3 N2H4 NH2OH N2 N2O NO NO2– NO2 NO3
– Cl– Cl2 ClO– ClO2
– ClO2 ClO2
– ClO3–
ClO4–
CO H2C2O4 C2O42–
C2H6 CH4 CO2 CO32–
PH3 P4 H3PO4 PO43–
H2S HS– S2– S6 SO2 SO3– SO3 S2O3
2– SO42–
H2O2
MnO2 KMnO4 MnO4– K2CrO4 CrO4
– K2Cr2O7 Cr2O7–
Review stoichiometry
aqueous solution reactions 12
Half ReactionsThese reactions explained during the lecture:
Zn = Zn2+ + 2 e–
Cu2+ + 2 e– = Cunet (electron transfer) Zn (s) + Cu2+ (aq) = Zn2+ (aq) + Cu (s)
For these half reactions,
Zn = Zn2+ + 2 e–
2 H+ + 2 e– = H2 get and explain the net reaction yourself
Explain how reactions proceed
aqueous solution reactions 13
Balance Half Equations
1. Identify the key element that undergoes an oxidation state change.
2. Balance the number of atoms of the key element on both sides.
3. Add the appropriate number of electrons to compensate for the change of oxidation state.
4. Add H+ (in acid medium), or OH- (in basic medium), to balance the charge on both sides of the half-reactions; and H2O, if necessary, to balance the equations.
Balance
MnO4 – + ____ + _____ Mn2+ + __ H2O
Page 9 of handout
aqueous solution reactions 14
Balance these half equations
Zn (s) Zn2+(aq)
Cu2+ (aq) Cu (s)
H2(g) H+ (aq)
I –(aq) I2
Fe2+ (aq) Fe3+ (aq)
SO32– (aq) SO4
2– (aq)
2 S2O32–(aq) S4O6
2–(aq) + 2e–1
Cr2O72–(aq) Cr3+ (aq)
I will illustrate the balance of these half reaction equations and those equations in other slides during the lecture. If you are not at my lecture, you should practice their balance to acquire your skills.
The textbook gives a slight different method to balance redox equations and please find out the difference. Both ways wok. You may use either method.
Work on these from time to time
aqueous solution reactions 15
Balance Redox Reaction equations
Add two half reaction equations so that you can cancel all electrons to obtain a balanced redox reaction equation
H2O2 + I – I2 + H2O
MnO4 – + H2O2 Mn2+ + O2
MnO4 – + SO3
2– Mn2+ + SO42–
MnO4 – + Fe2+ Mn2+ + Fe3+
Cr2O7 2– + UO2+ Cr3+ + UO2
2+
Work on these from time to time to refresh your skills.
aqueous solution reactions 16
Disproportionation ReactionsBalance disproportionation reaction (the same substance is both oxidized and reduced)
H2O2 2 H2O + O2
S2O32– SO4
2– + S (s)
S2O32– SO2 + S (s)
Work on these from time to time
aqueous solution reactions 17
Analyze and Learn the SkillsAnalyze this example and learn the skills to help you overcome any difficulty.
Task: Balance the equation: S2O32– SO4
2– + S (s)
Identify the element oxidized and reduced: oxidation states of S in S2O32– SO4
2– and S are +4, +6, and 0 respectively. S is both oxidized and reduced.
The oxidation half reaction: S2O32– SO4
2– + 8 e– (2 S from +2 +6, (2×4=8))The reduction half reaction: S2O3
2– + 4 e – (2S from +2 0, (2×2=4)) S
Balance the charge with H+ S2O32–SO4
2– + 8 e– + 10 H+ (both sides have 2-) S2O3
2– + 4 e – + 6 H+ S (both sides have 0)
Add water to balance: S2O32– + 5 H2O SO4
2– + 8 e– + 10 H+ S2O3
2– + 4 e – + 6 H+ S + 3 H2O
Make # of e the same: S2O32– + 5 H2O SO4
2– + 8 e– + 10 H+ 2 S2O3
2– + 8 e – + 12 H+ S + 6 H2O
The balanced equation: 3 S2O32– + 2 H+ SO4
2– + 4 S + 10 H+
Make sure you fill in the details too much to be included here!!!
aqueous solution reactions 18
Balance Redox Reaction in Basic Solutions
Redox reactions may have different products depends on the acidity (pH) of the solutions.
In basic solutions, there are more OH– ions than H+ ions. Thus, it is sensible to have OH– appearing in the equations than to have H+ ions.
Balance these reactions in a basic solution:
MnO4 – + CN – MnO2 + OCN –
Any one of several ways to assign oxidation states for CN works.
MnO4 – + SO3
2– MnO2 + SO42–
Practice balance these from time to time to polish you skills!
aqueous solution reactions 19
Oxidizing and Reducing Agents
Oxidizing agent or oxidant such as O2 or F2 is a substance that is able to oxidize other substances. It is reduced in the process (gains electron or decreases oxidation state).
Describe reducing agent or reductant
NH3 N2H4 NH2OH N2 N2O NO NO2 – NO2 NO3
–
Species Cannot be reduced further
Species Cannot be oxidized further
O x I d a n t
R e d u c t a n t
aqueous solution reactions 20
Titrations
Titration is a method used in volumetric analysis. The addition of a solution is carefully controlled so that stoichiometric amounts can be read from a burette.
Titration can be carried out for instantaneous or rapid reactions such as neutralization and oxidation reactions.
Explain these terms: neutralization,
titration,quivalence point,
half equivalence point, indicators
aqueous solution reactions 21
Conductance in Titration
conductance
V of NaOH added
Cl– Na+
H+ OH–
Conductance measurement of a HCl solution titrated by NaOH is shown:measured (total) conductancearea due to the ions labeled
Do all ions have the same conductance? Why or why not?
Why does the total conductance vary?
Is conductance of an ion depends on the concentration?
Explain physical properties of chemicals
aqueous solution reactions 22
Stoichiometry in Solution Chemistry
For titration calculations, the amount of reactant m is evaluated from the concentration C and volume V by
m = C * V
For example, when m1 amount of acid is neutralized by m2 amount of base, m1 = m1. For redox reactions, similar relationship can also be used, but the stoichiometric relationship should be kept in mind.
Amount in mmol = C in M * V in mL
aqueous solution reactions 23
Volumetric AnalysisA 5.00-mL sample of vinegar requires 38.08 mL of 0.1000 M NaOH solution to reach the equivalence point. What is the concentration of acetic acid in the vinegar by weight percent if its density is 1.01 g / mL?
Solution:
Net reaction: OH– + HC2H3O2 H2O + C2H3O2 – (aq)
38.08 mL OH–
5 mL vinegar0.1000 mol1000 mL
1 mol HC2H3O2 1 mol OH–
60.05 g HC2H3O2 1 mol HC2H3O2
1 mL vinegar1.01 g vinegar
= 0.0453 HC2H3O2 in vinegar
= 4.53 % HC2H3O2 in vinegarThe vinegar has 4.53 % of acetic acid by mass.
What’s the concentration of a 7% vinegar?
If you find this solution difficult to understand, use your own method to solve it
aqueous solution reactions 24
38.08 mL OH–
5 mL vinegar
0.1000 mol1000 mL
1 mol HC2H3O2 1 mol OH–
60.05 g HC2H3O2 1 mol HC2H3O2
1.01 g vinegar1 mL vinegar
= 0.0453 HC2H3O2 in vinegar
= 4.53 % HC2H3O2 in vinegar
What the concentration of a 7% vinegar?
A 5.00-mL sample of vinegar requires 38.08 mL of 0.1000 M NaOH solution to reach the equivalence point. What is the concentration of acetic acid in the vinegar by weight percent if its density is 1.01 g / mL?Solution: a slight variation and hope you find it easier to followNet reaction: OH– + HC2H3O2 H2O + C2H3O2
– (aq)
Mass of acetic acid
Mass of sample4.53 % ofHC2H3O2 in vinegar =
Another way of thinking
aqueous solution reactions 25
Chemical Analysis Application
How much 0.1000 M KMnO4 solution is required to reach the equivalence point in a titration of 1.00 g oxidize oxalic acid (oa = H2C2O4.2H2O)?
Solution: Redox reaction:2 MnO4
– + 5 H2C2O4 + 6 H+ = 2 Mn2+ + 8 H2O + 10 CO2 (balanced? Chk pls)
1.00 g oa1 mol oa
126 g oa
2 mol MnO4
5 mol oa
1000 mL
0.1000 mol= 31.75 mL MnO4
–
Do problem 5.97
Molar mass of H2C2O4.2H2O = 126 g mol-1
Note mole ratio in the balanced equation.
aqueous solution reactions 26
Back TitrationA 1.00-g sample containing MnO2 dissolved in solution is treated with 2.00 g of oxalic acid (oa = H2C2O4.2H2O). Then 50.00 mL 0.1000 M KMnO4 is required for the titration of the excess oa. What is the % MnO2 by mass?
Solution: Redox reaction:2 MnO4
– + 5 H2C2O4 + 6 H+ = 2 Mn2+ + 8 H2O + 10 CO2
H2C2O4 + MnO2 + 2 H+ = Mn2+ + 2 H2O + 2 CO2 (balanced? Chk pls)
50.00 mL MnO4
0.1000 mol MnO4
1000 mL
5 mol oa
2 mol MnO4
86.9 g MnO2
126 g oa
100 %
1.0 g Sample
126 g oa
1 mol oa= 1.575 g oa
(2.000 - 1.575) g oa = 29.0 % MnO2 by mass
Cool head 4 complicated problem, eh!
aqueous solution reactions 27
Review 1Sufficient amount of AgNO3 is placed in a 10.00 mL of tab water, and the AgCl solid is filtered and dried. The solid weighs 0.123 g. What is the concentration of chloride ion?
Solution: access and limiting reagent, and ppt
1 mol AgCl143.4 g AgCl
1 mol Cl-1 mol AgCl
0.123 g AgCl 10.00 mL
= 0.0858 mol / L of Cl–
1000 mL1 L
Express [Cl-] in mol and mass %.
aqueous solution reactions 28
Review 2A 0.1234-g sample (S) NaCl and sugar mixture contains 40% NaCl. When dissolved in water, the solution is treated with AgNO3. How much dry AgCl is the theoretical yield?
Solution: percentage analysis
40 g NaCl100 g S
1 mol AgCl58.5 g NaCl0.1234 g S
= 0.1323 g AgCl theoretical yield
143.4 g AgCl1 mol AgCl
Use the factors to help you think!
aqueous solution reactions 29
Review 3A 0.2345-g sample (S) NaCl and CaCl2 mixture contains 40% NaCl. When dissolved in water, the solution is treated with AgNO3. How much dry AgCl is the theoretical yield?
Solution:
0.2345*0.40 g NaCl = 0.2299 g AgCl 143.4 g AgCl58.5 g NaCl
Solve the same for a mixture of NaCl and KCl.
Find the percentage of NaCl if 0.5000 g AgCl is collected.
0.2345*0.60 g CaCl22*143.4 g AgCl
110 g CaCl2= 0.3668 g AgCl
(0.2299 + 0.3668) g AgCl = 0.5967 g AgCl
aqueous solution reactions 30
Review 4When 0.2345-g NaCl and CaCl2 mixture is dissolved in water, the solution is treated with AgNO3. The mass of dry AgCl collected is 0.5967 g. What is the percentage of NaCl in the mixture?
Solution: Assume the sample contains x fraction of NaCl0.2345 (x) g NaCl 143.4 g AgCl
58.5 g NaCl
Solve the same problem for 0.6000 instead of 0.5967 g AgCl.
In this problem, what are the min. and max. masses of AgCl? (0.5748 – 0.6114 g)
+ 0.2345 (1 – x) g CaCl22*143.4 g AgCl
110 g CaCl2= 0.5967 g AgCl
Solve for x in the equation: x = 0.40 = 40%
aqueous solution reactions 31
Review 5 - skills
obtain empirical formula from composition and combustion experiment
find molecular formula from empirical formula and molar mass
evaluate theoretical yield in a reaction, identify the limiting reagent
Identify limiting reagent and evaluation percent yield in a reaction
predict amounts of products or reagents required in reactions
find percent yield of a reaction but pay attention to limiting reagent
give concentration of common ions in a solution of several salts
calculate masses of reagents or products (AgCl) involving common ions
find percentage of a compound in a mixture by titration or precipitation
aqueous solution reactions 32
Review 6 – skill 2
Identify oxidation states and recognize reagent oxidized
balance redox reaction equations
evaluate quantities of reagents or products involving redox reactions
stoichiometry calculation in titration experiments paying attention to molar relationship such as H3PO4, Ca(OH)2, as well as redox reactions
evaluate quantities involving isotope composition of elements
calculate one of density, mass and volume in solid, liquid, and gas
name inorganic compounds
write proper net ionic equation of reaction (know your spectator ions)
aqueous solution reactions 33
TA Hours & Rooms – fall 03The Tutors handle the tutorial periods for CHEM 120/121 but they can also provide assistance to individuals or small groups on a drop-in basis according to the following schedule. (i.e. One of the Tutors will be in each room for the specified period. You can drop in at any time during that period to get some help.)
Day Time Room*Monday 12:30-1:20 PHY 313Monday 1:30-2:20 MC 4062Monday 2:30-3:20 PHY 150Wednesday 12:30-3:20 PHY 313Wednesday 1:30-2:20 MC 4060
* These rooms are for one-on-one tutorial, not tutors office.