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Final

CHEM403 Lecture 4: lab lecture 4Exam


Department
Chemistry
Course Code
CHEM403
Professor
Winans
Study Guide
Final

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Grace Roy and Kella Psillas
Lab 4: Ionic Precipitation Reactions
Group Portion:
1. When the KI and Pb(NO3)2 were placed on opposite sides of the drop of water, a yellow
thread-like solid formed in the middle of the drop after the two crystals began to dissolve.
2. 2KI (aq) + Pb(NO3)2 (aq) β†’ 2KNO3 (aq) + PbI2 (s)
Pb2+ (aq) + 2I+ (aq) β†’ PbI2 (s)
3. The reaction that was observed is a precipitate reaction, where two ions form an insoluble
ionic compound that falls out of an aqueous solution to form a solid.
4. Chemical names and formulas:
Name
Chemical Formula
Hydrogen Sulfate
H2SO4
Sodium Phosphate
Na3PO4
Sodium Hydroxide
NaOH
Sodium Carbonate
Na2CO3
Silver Nitrate
AgNO3
Potassium Iodide
KI
Lead (II) Nitrate
Pb(NO3)2
Hydrogen Chloride
HCl
Iron Chloride
FeCl3
Copper (II) Sulfate
CuSO4
Barium Chloride
BaCl2
Ammonium Hydroxide
NH4OH
Nitric Acid
HNO3
Aluminum Chloride
AlCl3
5. See attached
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6.
Reactant 1
Reactant 2
Chemical Equation
Na3PO4
(aq)
AlCl3 (aq)
2Na3PO4 (aq) + 2AlCl3 (aq) β†’ 6NaCl (aq) + 2AlPO4 (s)
Al3+ (aq) + PO43- (aq) β†’ AlPO4 (s)
NaOH
(aq)
AlCl3 (aq)
3NaOH (aq) + AlCl3 (aq) β†’ 3NaCl (aq) + Al(OH)3 (s)
Al3+ (aq) + 3OH- (aq) β†’ Al(OH)3 (s)
Na2CO3
(aq)
AlCl3 (aq)
3Na2CO3 (aq) + 2AlCl3 (aq) β†’ 3NaCl (aq) + Al2(CO3)3 (s)
2Al3+ (aq) + 3CO32- (aq) β†’ Al2(CO3)3 (s)
AgNO3
(aq)
AlCl3 (aq)
3AgNO3 (aq) + AlCl3 (aq) β†’ 3AgCl (s) + Al(NO3)3 (aq)
Ag+ (aq) + Cl- (aq) β†’ AgCl (s)
Pb(NO3)2
(aq)
AlCl3 (aq)
3Pb(NO3)2 (aq) + 2AlCl3 (aq) β†’ 3PbCl2 (s) + 2Al(NO3)3 (aq)
Pb2+ (aq) + 2Cl- (aq) β†’ 3PbCl2 (s)
FeCl3 (aq)
AlCl3 (aq)
FeCl3 (aq) + AlCl3 (aq) β†’ FeCl3 (aq) + AlCl3 (aq)
No precipitate reaction (dark yellow clear mixture after reaction)
CuSO4
(aq)
AlCl3 (aq)
3CuSO4 (aq) + 2AlCl3 (aq) β†’ Al2(SO4)3 (aq) + 3CuCl2 (aq)
No precipitate reaction (light blue after reaction)
NH4OH
(aq)
AlCl3 (aq)
3NH4OH (aq) + AlCl3 (aq) β†’ 3NH4Cl (aq) + Al(OH)3 (s)
Al3+ (aq) + 3OH- (aq) β†’ Al(OH)3 (s)
Na2CO3
(aq)
NH4OH
(aq)
Na2CO3 (aq) + 2NH4OH (aq) β†’ 2NaOH (aq) + (NH4)2CO3 (aq)
No precipitate reaction (white clumps formed after reaction)
AgNO3
(aq)
NH4OH
(aq)
AgNO3 (aq) + NH4OH (aq) β†’ AgOH (s) + NH4NO3 (aq)
Ag+ (aq) + OH- (aq) β†’ AgOH (s)
Pb(NO3)2
(aq)
NH4OH
(aq)
Pb(NO3)2 (aq) + 2NH4OH (aq) β†’ Pb(OH)2 (s) + NH4NO3 (aq)
Pb2+ (aq) + 2OH- (aq) β†’ Pb(OH)2 (s)
FeCl3 (aq)
NH4OH
(aq)
FeCl3 (aq) + 3NH4OH (aq) β†’ Fe(OH)3 (s) + 3NH4Cl (aq)
Fe3+ (aq) + 3OH- (aq) β†’ Fe(OH)3 (s)
CuSO4
(aq)
NH4OH
(aq)
CuSO4 (aq) + 2NH4OH (aq) β†’ Cu(OH)2 (s) + (NH4)2SO4 (aq)
Cu2+ (aq) + 2OH- (aq) β†’ Cu(OH)2 (s)
BaCl2 (aq)
NH4OH
(aq)
BaCl2 (aq) + 2NH4OH (aq) β†’ Ba(OH)2 (aq) + 2ClNH4 (aq)
No precipitate reaction (white clumps formed after reaction)
H2SO4
(aq)
BaCl2 (aq)
H2SO4 (aq) + BaCl2 (aq) β†’ 2HCl (aq) + BaSO4 (s)
Ba2+ (aq) + SO42- (aq) β†’ BaSO4 (s)
Na3PO4
(aq)
BaCl2 (aq)
2Na3PO4 (aq) + 3BaCl2 (aq) β†’ 6NaCl (aq) + Ba3(PO4)2(s)
3Ba2+ (aq) + 2PO43- (aq) β†’ Ba3(PO4)2 (s)
NaOH
(aq)
BaCl2 (aq)
2NaOH (aq) + BaCl2 (aq) β†’ 2NaCl (aq) + Ba(OH)2 (s)
Ba2+ (aq) + 2OH- (aq) β†’ Ba(OH)2 (s)
*according to solubility rules, Ba(OH)2 is soluble, but the reaction that
occurred resulted in a frosted white appearance to mixture, which
flaked when disturbed with a pipette.
Na2CO3
(aq)
BaCl2 (aq)
Na2CO3 (aq) + BaCl2 (aq) β†’ 2NaCl (aq) + BaCO3 (s)
Ba2+ (aq) + CO32- (aq) β†’ BaCO3 (s)
AgNO3
(aq)
BaCl2 (aq)
2AgNO3 (aq) + BaCl2 (aq) β†’ 2AgCl (s) + Ba(NO3)2 (aq)
Ag+ (aq) + Cl- (aq) β†’ AgCl (s)
KI (aq)
BaCl2 (aq)
2KI (aq) + BaCl2 (aq) β†’ 2KCl (aq) + BaI2 (aq)
No precipitate reaction (pale yellow and clear after reaction)
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