Dr. Talmage
1/17/12
A4
Double Replacement Reactions
Objective: To recognize and infer possible reactions and precipitant formations between different ionic substances.
Procedure: In this lab we mixed many different substances to see if they formed a double replacement reaction. We also looked for precipitants that were formed from the mixing of the different substances. We used barium nitrate, potassium hydroxide, sodium sulfate, magnesium nitrate, aluminum sulfate, and iron (III) chloride in set one. In set two we used potassium chloride, sodium hydroxide, magnesium nitrate, barium chloride, sodium sulfate, and magnesium sulfate. For each set, we mixed two drops of one compound in five wells of a spot plate. We then added two drops of all the other substances to the compound. We repeated this procedure for set two. If a precipitant formed from any solution, we recorded the color on our data table. If no precipitant formed, we recorded NR. After mixing and recording all the compounds we rinsed to spot plate thoroughly with water.
Data Tables
Set #1
Ba(NO3)2
Na2SO4
Al2(SO4)3
KOH
MgCl2
FeCl3
Ba(NO3)2
Milky ppt
Milky ppt
NR
NR
Yellow ppt
Na2SO4
NR
NR
NR
Peach ppt
Al2(SO4)3
NR
NR
Orange ppt
KOH
NR
Carrot Orange ppt
MgCl2
Lemon yellow ppt
FeCl3
Set #2
KCl
MgCl2
Na2SO4
NaOH
BaCl2
MgSO4
KCl
NR
NR
NR
NR
NR
MgCl2
NR
NR
Cloudy ppt
NR
Na2SO4
NR
Cloudy ppt
NR
NaOH
NR
NR
BaCl2
Cloudy ppt
MgSO4
Questions:
1. On the attached sheet
2. A precipitate forms when a solid is made from two reactants combining together.
3. One example would be mixing KCI with KCI, in this case you wouldn’t get a precipitant because you are combining two of the same things. Another example would be combining a metal and a nonmetal, such as NaSo4 and KCl. There was no precipitate.
4. In a net ionic equation you break apart the entire beginning of
A4
Double Replacement Reactions
Objective: To recognize and infer possible reactions and precipitant formations between different ionic substances.
Procedure: In this lab we mixed many different substances to see if they formed a double replacement reaction. We also looked for precipitants that were formed from the mixing of the different substances. We used barium nitrate, potassium hydroxide, sodium sulfate, magnesium nitrate, aluminum sulfate, and iron (III) chloride in set one. In set two we used potassium chloride, sodium hydroxide, magnesium nitrate, barium chloride, sodium sulfate, and magnesium sulfate. For each set, we mixed two drops of one compound in five wells of a spot plate. We then added two drops of all the other substances to the compound. We repeated this procedure for set two. If a precipitant formed from any solution, we recorded the color on our data table. If no precipitant formed, we recorded NR. After mixing and recording all the compounds we rinsed to spot plate thoroughly with water.
Data Tables
Set #1
Ba(NO3)2
Na2SO4
Al2(SO4)3
KOH
MgCl2
FeCl3
Ba(NO3)2
Milky ppt
Milky ppt
NR
NR
Yellow ppt
Na2SO4
NR
NR
NR
Peach ppt
Al2(SO4)3
NR
NR
Orange ppt
KOH
NR
Carrot Orange ppt
MgCl2
Lemon yellow ppt
FeCl3
Set #2
KCl
MgCl2
Na2SO4
NaOH
BaCl2
MgSO4
KCl
NR
NR
NR
NR
NR
MgCl2
NR
NR
Cloudy ppt
NR
Na2SO4
NR
Cloudy ppt
NR
NaOH
NR
NR
BaCl2
Cloudy ppt
MgSO4
Questions:
1. On the attached sheet
2. A precipitate forms when a solid is made from two reactants combining together.
3. One example would be mixing KCI with KCI, in this case you wouldn’t get a precipitant because you are combining two of the same things. Another example would be combining a metal and a nonmetal, such as NaSo4 and KCl. There was no precipitate.
4. In a net ionic equation you break apart the entire beginning of