Copper and silver nitrate lab answers

Lab 8 - Oxidation-Reduction Activity Series

Nisaa Sarwar

3/20/2017 @ 1:00 p.m.

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Chemistry 1105 Net-03

Nisaa Sarwar

Unit 8

Purpose: ​The purpose of this lab is to observe and differentiate between chemical

reactions and to learn how to write balanced chemical equations for them.

Procedure:

Experiment 1:

1. Make sure you put on your gloves and goggles before you start.

2. First, take a test tube, the silver nitrate, the copper pieces, and the plastic

tweezers and set them aside.

3. Observe and record the initial appearance of the silver nitrate and the copper.

4. Then, using the plastic tweezers, add two pieces of copper into the test tube.

5. Next, add all the silver nitrate into the test tube and throw out the empty bottle.

6. Observe and record the reaction for up to a minute and then describe the

appearance of all solid, liquid, and gas in the test tube.

7. Let the reactions go on for another 30 minutes, then observe and record the

appearance of the all the solid, liquid, and gas.

8. Write the balanced chemical equation for the redox reaction on a sheet of paper,

including the oxidation numbers and total charge. Take a photo and upload it.

9. Figure out which one of the elements has been reduced and which one is the

spectator ion. Record your observations.

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Unit 8

10. Figure out which element was the oxidizing agent and which was the reducing

agent in the experiment. Record your observations.

11. Clean up the materials used properly.

Experiment 2:

1. First, take the 24 well plate and place it on top of a paper with labels for the well

plate. Label wells A1, A2, B1, B2, C1, and C2.

2. Next, put a piece of copper in both well plate A1 and well plate A2.

3. Then, take the pipet with the lead (II) nitrate and cut off the tip of the pipette. Add

15 drops of the lead (II) nitrate to well A1.

4. Observe and record the chemical reaction in well A1 after a minute.

5. Let the reaction in well A1 continue for 30 more minutes.

6. Meanwhile, cut off the tip of the pipette containing the zinc nitrate. Add 15 drops

of zinc nitrate to well A2.

7. Observe and record the chemical reaction in well A2 after a minute.

8. Take the plastic tweezers to grab two pieces of lead and place it on a piece of

paper towel.

9. Then, take a nail filer and scrape the top of the lead to take off the rust.

10. Put the two pieces of lead, one in each, wells B1 and B2.

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Unit 8

11. Dispose of the paper towel with the lead leftovers on it. Also, throw out the nail

filer.

12. Take your gloves off inside out and throw them away. Wash your hands with

soap and dry them with paper towels, throwing the paper towels out afterwards.

13. Put on a new pair of gloves.

14. Next, take the pipet with the copper (II) sulfate and cut off the tip. Add 15 drops

of the copper (II) sulfate to well B1. Observe and record the reaction after a

minute.

15. Then, add 15 drops of Zn(NO3)2 to well B2. Observe and record the reaction

after a minute.

16. Put one piece of mossy zinc in well C1 and one piece in well C2.

17. Add 15 drops of CuSO4 to well C1. Observe and record the reaction after a

minute.

18. Add 15 drops of Pb(NO)2 to well C2. Observe and record the reaction after a

minute.

19. After 30 minutes, observe and re-record all the reactions so far.

20. Fill in the data tables with the all observations.

21. Write balanced chemical equations for all the reactions that occurred, including

the oxidation numbers and the total charge. Take a picture and upload it.

22. Clean up the materials used properly.

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Unit 8

Observation & Data:

Data Table 1: Redox Reaction of Copper and Silver Nitrate

Initial

Observations

before Beginning

The copper pieces are a bronzish color while the silver nitrate is

clear.

Observations

First, the copper turned white with bubbles and then black. Also,

it kind of fluffed up (like a pill when it dissolves). The liquid is

clear.

Observations

after 30 min

The pieces combined and turned crystallized. It turned a

combination of white, brown, and black in color. The liquid also

turned into a slight light blue green color.

Element that is

Oxidized

Copper

Element that is

Reduced

Silver

Spectator Ion None

Oxidizing Agent Copper

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Unit 8

Reducing Agent Silver

Data Table 2: Redox Reactions of Copper, Lead, and Zinc

Solid Metal

Well ID

Solution

Immediate

Observation

30 Minute

Observation

Cu

A1

Pb(NO​3​)​2

The liquid is clear while

the copper is bronze in

color.

There was no

change.

Cu

A2

Zn(NO​3​)​2

The liquid is clear while

the copper is bronze in

color.

There was no

change.

Pb

B1

CuSO​4

There are a few

bubbles that form

around the lead, which

turns bronze in color.

The lead starts to

rust.

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Unit 8

Pb

B2

Zn(NO​3​)​2

The lead is silver in

color.

There was no

change.

Zn

C1

CuSO​4

The zinc turned reddish

from the top.

The zinc was black

with a little bit of red

on the top.

Zn

C2

Pb(NO​3​)​2

The zinc turns black.

The zinc becomes

dark grey from the

top.

Data Table 3: Potential Redox Reactions and Chemical Equations

Metal and Metallic Solution Reaction Occurred?

Cu + Pb(NO​3​)​2 None

Cu + Zn(NO​3​)​2 None