It also includes; Nitrates such as Lead Nitrate, Copper Nitrate, Magnesium Nitrate, Zinc Nitrate, and Iron Nitrate, and Tin chloride. In this activity lab it includes lab lab equipment, the metals, and the nitrates. We used less metals and nitrates than were available in our Lab. We used Magnesium, Zinc, Lead, Copper, and Iron for our metals. We used Magnesium Nitrate, Zinc Nitrate, Lead Nitrate, Copper Nitrate, Silver Nitrate and Iron Nitrate as our nitrates. For lab equipment we used beakers, pipets, a scooper,
Nick Pearlman, Dylan Whitney, Garret Rohan
Background
The Activity Series Lab is a lab that shows that reactivity of metals. The experiment allowed the viewer to see simple metals being changed in Nitrate solutions using redox reactions. We we are able to place metals in aqueous nitrates and observe their reactions. Redox reactions made this possible as the Metals and Nitrates used in the reactions gave and took electrons to produce the solution. A good example of this is when Zinc was placed in Lead nitrate. Before the reaction took place, Zn was a solid metal. But after the reaction began to take place, it slowly began to change color and appear to dissolve. The redox reaction took place in a very visible manner. This is what the activity series lab was meant to do; show redox reactions take place.
Materials
Metals
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Nitrates
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Other
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Magnesium
|
Magnesium nitrate
|
Water
|
Zinc
|
Zinc nitrate
|
Beaker
|
Copper
|
Copper nitrate
|
Tray
|
Iron
|
Iron nitrate
|
Scooper
|
Lead
|
Lead nitrate
|
Pipet
|
Silver nitrate
|
Tweezers
|
Objective
Our two primary objectives in this experiment were to discover the reactivity of various metals when placed in various nitrates and also to gain a better understanding of redox reactions and how to write equations for them.
Procedure
1. Acquire the needed metals, nitrates, and lab equipment.
2. Fill three sections of the tray with Magnesium nitrate. Place a strip of Magnesium, Zinc, and Copper in the individual sections of the tray (one strip in each section). Observe and record the reactions or lack thereof.
3. Repeat step two a total of three more times, but use Zinc nitrate, Copper nitrate, and Silver nitrate instead if the Magnesium nitrate.
4. Rinse tray and other pieces of lab equipment after gingerly disposing of the solutions.
5. Fill 16 sections of the tray, four each with Iron nitrate, Zinc nitrate, Copper nitrate, and Lead nitrate. Place a strip of Iron, Copper, Zinc, and Lead in the sections of the tray (each metal in one section of one section of each nitrate. One strip in each section). Observe and record the reactions or lack thereof.
Data
Trial 1
Mg(NO3)2
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Zn(NO3)2
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Cu(NO3)2
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Ag(NO3)
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Mg
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No reaction
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Mg turned a lighter grey almost like Zn
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Mg appeared to have black and white spots
|
Mg become black and fuzzy looking
|
Cu
|
No reaction
|
No reaction
|
No reaction
|
Cu turned brown and looked fuzzy
|
Zn
|
No reaction
|
No reaction
|
Zn appears to have a slightly black tint
|
Zn is very dark black and looks as if dissolving
|
Ag
|
N/A
|
N/A
|
N/A
|
N/A
|
Trial 2
Fe(NO3)2
|
Zn(NO3)2
|
Cu(NO3)2
|
Pb(NO3)2
| |
Fe
|
Fe darkened the color of the Fe(NO3)2
|
No Reaction
|
Cu(NO3)2 turned from a blue to a yellow
|
No Reaction
|
Cu
|
Cu appeared to be a lighter color almost a pink
|
No Reaction
|
No Reaction
|
No Reaction
|
Zn
|
Zn had a yellow tint, Fe(NO3)2 became darker
|
No Reaction
|
No Reaction
|
Zn looked black and looked as if disintegrating
|
Pb
|
No Reaction
|
No Reaction
|
Pb turned black, Cu(NO3)2 after had a green tint
|
No Reaction
|
Most to least reactive:
1. Magnesium: Reacted more nitrates than any of the other metals.
2. Zinc: Reacted consistently with many of the nitrates.
3. Iron: Reacted with few number of nitrates, but did react with Fe(NO3)2, so is more reactive than Lead
4. Lead: Reacted with few number of nitrates, but didn’t react with Fe(NO3)2, so is less reactive than Iron
5. Copper: Reacted with less nitrates than any of the other metals.
Reactions
Mg+Mg(NO3)2---->
Mg+Mg(NO3)2
|
Mg+Zn(NO3)2---->
Zn+Mg(NO3)2
|
Mg+Cu(NO3)2---->
Cu+Mg(NO3)2
|
Mg+Ag(NO3)2---->
Ag+Mg(NO3)2
|
Cu+Mg(NO3)2---->
Cu+Mg(NO3)2
|
Cu+Zn(NO3)2---->
Cu+Zn(NO3)2 |
Cu+Cu(NO3)2---->
Cu+Cu(NO3)2
|
Cu+Ag(NO3)2---->
Ag+Cu(NO3)2
|
Zn+Mg(NO3)2---->
Zn+Mg(NO3)2
|
Zn+Zn(NO3)2---->
Zn+Zn(NO3)
|
Zn+Cu(NO3)2---->
Cu+Zn(NO3)2
|
Zn+Ag(NO3)2---->
Ag+Zn(NO3)2
|
N/A
|
N/A
|
N/A
|
N/A
|
Fe+Fe(NO3)2---->
Fe+Fe(NO3)2
|
Fe+Zn(NO3)2---->
Fe+Zn(NO3)2
|
Fe+Cu(NO3)2---->
Cu+Fe(NO3)2
|
Fe+Pb(NO3)2---->
Fe+Pb(NO3)2
|
Cu+Fe(NO3)2--->
Fe+Cu(NO3)2
|
Cu+Zn(NO3)2---->
Cu+Zn(NO3)2
|
Cu+Cu(NO3)2---->
Cu+Cu(NO3)2
|
Cu+Pb(NO3)2---->
Cu+Pb(NO3)2
|
Zn+Fe(NO3)2---->
Fe+Zn(NO3)2
|
Zn+Zn(NO3)2----->
Zn+Zn(NO3)2
|
Zn+Cu(NO3)2---->
Zn+Cu(NO3)2
|
Zn+Pb(NO3)2---->
Pb+Zn(NO3)2
|
Pb+Fe(NO3)2----->
Pb+Fe(NO3)2
|
Pb+Zn(NO3)2---->
Pb+Zn(NO3)2
|
Pb+Cu(NO3)2---->
Cu+Pb(NO3)2
|
Pb+Pb(NO3)2---->
Pb+Pb(NO3)2
|
Sources:
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