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Topic 5
Ions in Aqueous Solutions (Net Ionic Equations)
Keys, Group Work;
Homework Assignments
Group Work Keys
• 5.1 Ions in Solution
• 5.2 Solubility Chart #1
• 5.3 Solubility Chart #2
• 5.4 Net Ionic Equations,
Precipitation Reactions
• 5.5 Net Ionic Equations,
Acid Base Reactions
Homework
Assignments,
Kotz & Treichel,
Chapter 5: 5.1-5.6
Slides 19, 20
Key,Group Work 5.1: Electrolytes in
Solution
Compound
Type
#Ions in
Solution
Compound Type
# Ions in
Solution
HClO4
ACID
1 H+
1 ClO4-
Cu(ClO4)2
Salt
1 Cu2+
2 ClO4-
Ca(OH)2
Base
1 Ca2+
2 OH-
Ca (NO3) 2
Salt
1 Ca2+
2 NO3-
KHSO4
Salt
1 K+
1 HSO4-
NH4H2PO4
Salt
1 NH4+
1 H2PO4-
Fe2(SO4)3
Salt
2 Fe3+
3 SO42-
HBrO3
Acid
1 H+
1 BrO3-
Salt
1 Sn4+
4 Cl-
Ni(CH3CO2)2 Salt
1 Ni2+
SnCl4
2 CH3CO2
Key, Group Work 5.2
Formula
Name
FeCO3
Iron(II) Carbonate
NO, carbonate
K2CO3
Yes, K+
Co3(PO4)2
Potassium
Carbonate
Ammonium
Phosphate
Cobalt(II) Phosphate
Mg(NO3)2
Magnesium Nitrate
Yes, nitrate
AgCl
Silver Chloride
NO, exception
CuI2
Copper (II) Iodide
Yes, iodide
Cr2(SO4)3
Chromium(III) Sulfate
Yes, sulfate
(NH4)3PO4
H2O Soluble?
Yes, NH4+
NO, phosphate
KEY, GROUP WORK 5.3
Bi(ClO4)3
Ag Br
CdSO4
Zn(NO3)2
Bismuth(III) Perchlorate
Silver Bromide
Cadmium Sulfate
Zinc Nitrate,
Yes, Perchlorate
No, Exception
Yes, Sulfate
Yes, Nitrate
KEY, GROUP WORK 5.3, CONTINUED
Nickel(II) Nitrate
Potassium Permanganate
Barium Sulfate
No
Aluminum Oxide
No
Magnesium Nitride
No
Ni(NO3)2
KMnO4
BaSO4
Al2O3
Mg3N2
Yes (nitrate)
Yes (K+)
(exception)
(oxide)
(Nitride)
KEY, GROUP WORK 5.4
b) K2CO3 (aq) + NH4NO3 (aq) ---> ?
K+ (no ppt)
NH4+ (no ppt)
CO32- (ppt???)
NO3- (no ppt)
NO REACTION OCCURS
a) Na2CO3 (aq) + Al(NO3)3 ( aq) ---> ?
Na+ (no ppt)
Al3+ (ppt???)
CO32- (ppt???)
NO3- (no ppt)
REACTION OCCURS!
Key, Group Work 5.4, b) continued
2. Complete and double check the product formulas:
Al 3 + + (CO3)2- ---> Al2(CO3)3
Na+
Charge
per ion
+
(NO3)- ---> NaNO3
1+ 1NaNO3
1+ 1-
3+
2-
Al2(CO3)3
6+
6-
Total
charge
Unbalanced Equation:
Na2CO3 (aq) + Al(NO3)3 ( aq) ---> NaNO3 ( aq) + Al2(CO3)3(s)
Key, Group Work 5.4, b) continued
3. Balance:
3Na2CO3 (aq) + 2Al(NO3)3 ( aq) --->6 NaNO3 ( aq) + Al2(CO3)3(s)
4. Total ionic equation:
[6Na+ (aq) + 3 CO32- (aq)] + [2 Al3+ (aq) + 6 (NO3) - ( aq)] --->
[6Na+ (aq) +6 (NO3) - ( aq)] + Al2(CO3)3(s)
5. Net Ionic Equation:
2 Al3+ (aq) + 3 CO32- (aq) ---> Al2(CO3)3(s)
Key, Group Work 5.4, c)
1c) CrCl3 (aq) + K3PO4 (aq) --->?
1. c) CrCl3 (aq) + K3PO4 (aq) ---> ?
Cr3+ (ppt???)
K+ (no ppt)
Cl- (generally soluble)
PO43- (ppt???)
REACTION OCCURS!
Key, Group Work 5.4, c) continued
2. Complete and double check the product
formulas:
Cr 3 + + PO43- ---> CrPO4
K+
+
Cl- ---> KCl
1+ 1-
3+
3-
KCl
CrPO4
1+ 1-
3+
3-
Unbalanced Equation:
CrCl3 (aq) + K3PO4 (aq) --->? KCl
( aq)
+ CrPO4 (s)
Key, Group Work 5.4, c) continued
3. Balance:
CrCl3 (aq) + K3PO4 (aq) ---> 3 KCl
( aq)
+ CrPO4 (s)
4. Total ionic equation:
[ Cr3+ (aq) + 3 Cl- (aq)] + [3 K+ (aq) + PO43 - ( aq)] --->
[3 K+ (aq) + 3 Cl- ( aq)] + CrPO4 (s)
5. Net Ionic Equation:
Cr3+ (aq) + PO43 - (aq) ---> CrPO4 (s)
Key, Group Work 5.5, #1
1. Fe2O3 (s) + HCl(aq) ---> ? -----> H2O + salt
salt: Fe3+
+ Cl- ----> FeCl3
Unbalanced:
Fe2O3 (s) + HCl(aq) ---> FeCl3 + H2O
Balanced:
Fe2O3 (s) + 6 HCl(aq) ---> 2 FeCl3 + 3 H2O
Key, GW 5.5, #1, continued
Fe2O3 (s) + 6 HCl(aq) ---> 2 FeCl3 + 3 H2O
Total Ionic:
Fe2O3 (s) + 6 H+ (aq) + 6 Cl- (aq) -----> 2 Fe3+ (aq)
+ 6 Cl- (aq) + 3 H2O (l)
Net Ionic:
Fe2O3 (s) + 6 H+ (aq) -----> 2 Fe3+ (aq) + 3 H2O (l)
Key, Group Work 5.5, #2
2. H2CO3 (aq) + KOH (aq) --->? -----> H2O + salt
salt: CO32-
+
K+ -----> K2CO3
Unbalanced:
H2CO3 (aq) + KOH (aq) ---> H2O(l) + K2CO3 (aq)
Balanced:
H2CO3 (aq) + 2 KOH (aq) --->2 H2O(l) + K2CO3 (aq)
Key, Group Work 5.5, #2, continued
H2CO3 (aq) + 2 KOH (aq) --->2 H2O(l) + K2CO3 (aq)
Total Ionic:
H2CO3 (aq)
+ 2 K+ (aq) + 2 OH- (aq) -----> 2 H2O (l)
+ 2 K+ (aq) + CO32- (aq)
Net Ionic:
H2CO3 (aq) + 2 OH- (aq) -----> 2 H2O (l) + CO32- (aq)
Key, Group Work 5.5, #3
3. H2SO4 (aq) + Ba(OH)2 (s) -----> ? -----> H2O + salt
salt: SO42- + Ba2+ ----> BaSO4
Unbalanced:
H2SO4 (aq) + Ba(OH)2 (s) -----> H2O(l) + BaSO4 (s)
Balanced:
H2SO4 (aq) + Ba(OH)2 (s) -----> 2 H2O(l) + BaSO4 (s)
Key, Group Work 5.5, #3, continued
H2SO4 (aq) + Ba(OH)2 (s) -----> 2 H2O(l) + BaSO4 (s)
Total Ionic:
2 H+ (aq) + SO42- (aq) + Ba(OH)2 (s) -----> 2 H2O(l)
+ BaSO4 (s)
No canceling spectators!
Net Ionic: Same as Total Ionic!
Chapter 5: Ions in Aqueous Solutions
Assignments
Sections 5.1-5.6 Net Ionic Equations: Double
Replacement Precipitation, Acid Base, Gas Forming
Reactions
• Study carefully Chapter 5, Sections 5.1- 5.6, p. 179-203
• Review chapter highlights, p. 228, first 9
Memorize:
• chart of predictably soluble salts, slide #23, 24
• chart of strong acids (structure, name) slide #36
• chart of weak acids (structure, name) slide #37
Written Assignments, Chapter 5 (5.1-5.6)
In Chapter Exercises:
#5.1- 5.9
Chapter 5“study questions” p. 229-234:
4, 6, 8; all even: 18-30; 34, 36, 48, 50, 52, 92, 94