Wendy Kim 1A
Lab Science 9
Ms. Nakai
Double Replacement Reaction
Problem
Why does Copper (II) Nitrate show visible reactions with Sodium Carbonate but not with
Sodium Chloride?
Hypothesis
If Copper (II) Nitrate is mixed with sodium carbonate, the reactions would be visible, but not
with sodium chloride because the characteristics of each element are different.
Experimental Method
Each of the chemicals will be mixed with ever single other solutions. Group A chemicals would
be independent variables and group B chemicals would be dependent variables. Photographs
would be taken during the experiment. For safety, wearing aprons, safety goggles, and
rubber gloves are necessary.
Procedure:
Materials Needed:
Chemicals
0.1M solutions of the following:
Group A
Copper (II) Nitrate
Nickel (II) Nitrate
Lead (II) Nitrate
Cobalt (II) Nitrate
Nitric Acid
Silver Nitrate
Aluminum Nitrate
Iron (III) Nitrate
Group B
Sodium Carbonate
Sodium Sulfate
Ammonium Hydroxide
Sodium Chloride
EDTA
Sodium Iodide
Sodium Thiocyanate
Sodium Chromate
Sodium Dichromate
Sodium Hydroxide
Demineralized Water
*Highlighted chemicals are the ones that I used for my hypothesis.
Hardware
96-well mirco plate
Pipettes
1. The objective of this experiment is to mix each of the reagents listed above from
GROUP A with each of the reagents from GROUP B. Arrange the 96-well micro plate
so that the lettered rows are on the left and the numbered columns are at the top.
2. Place 4 drops of Copper (II) Nitrate in each of the numbered wells in row A. After
rinsing your pipette, fill the wells in Row B with 4 drops of Nickel (II) nitrate. Rinse your
pipette again and continue in a similar manner using all of the solutions from GROUP
A.
3. When all of the rows have been given the particular reagent assigned from GROUP A,
begin to add 4 drops of each of the reagents from GROUP B, one reagent to each
column. Rinse your pipette between samples so that unwanted contamination does not
occur. For example, Sodium Carbonate is added to each well in column 1; Sodium
Sulfate is added to each of the wells in column 2. In this manner each of the
compounds in GROUP A is mixed with each of the compounds in GROUP B.
4. On the enclosed data sheet, record any combination that showed any form of
reactivity and indicate the form of that activity (e.g., gas, ppt, color change, etc.)
5. Write and balance a double replacement equation for each of the combinations that
showed any type of reactivity. You may have to predict the products, using the
method previously discussed.
Data Collection
Copper Nitrate
Nickel Nitrate
Lead Nitrate
Cobalt Nitrate
Nitric Acid
Silver Nitrate
Aluminum
Nitrate
Iron Nitrate
Sodium
Carbonate
Thick precipitate
formed
Thick precipitate
formed
Thick precipitate
formed
Thick precipitate
formed
No reaction
Thick precipitate
formed (white)
Sodium Sulfate
Precipitate
formed (white)
Precipitate
formed (turns
darker)
No reaction
Sodium Iodide
Copper
Nitrate
Nickel
Nitrate
Lead
Nitrate
Turns green,
yellow, forms
orange
precipitate
No reaction
Turns clear
No reaction
Thick precipitate
formed
No reaction
No reaction
No reaction
No reaction
Sodium
Thiocyanate
Turns green
No reaction
Turns bright
yellow, forms
precipitate
No reaction
Cobalt
Nitrate
No reaction
No reaction
Nitric Acid
Silver
Nitrate
No reaction
Forms palegreen
precipitate
No reaction
Precipitate
formed
Aluminum
Nitrate
No reaction
No reaction
Iron Nitrate
Turns darker
Forms layer of
dark, opaque
red
Ammonium
Hydroxide
Slight precipitate
formed
No reaction
Sodium
Chloride
No reaction
EDTA
No reaction
Turns blue
Turns blue
No reaction
No reaction
Turns blue,
precipitate formed
No reaction
Slight precipitate
(white)
No reaction
No reaction
No reaction
Turns opaque
white,
precipitate
No reaction
No reaction
Precipitate
formed
No reaction
No reaction
Slight precipitate
formed
Precipitate formed,
turns darker
Turns bluer
No reaction
Sodium
Chromate
Turns dark
yellow,
precipitate
formed
Turns yellowgreen
Turns bright
yellow,
precipitate
formed
Turns orangebrown
Sodium
Dichromate
Turns dark
yellow, slight
precipitate
Sodium
Hydroxide
Precipitate
formed
Demineralized
Water
No reaction
Turns dark
yellow
Turns bright
yellow,
precipitate
formed
Turns orange
No reaction
No reaction
Precipitate
formed
No reaction
No reaction
Turns yellow
Turns dark
red,
precipitate
formed
Turns yellow,
precipitate
formed
Turns orange,
precipitate
formed
Turns yellow
Turns dark
red-brown,
precipitate
formed
Turns yellow
(no
precipitate)
Turns orangeyellow,
precipitate
formed
Turns blue,
precipitate
formed
No reaction
Turns brown,
precipitate
formed
Slight
precipitate
formed
Turns dark
orangeyellow,
precipitate
No reaction
No reaction
No reaction
No reaction
Data Processing
1: Reactions of Copper Nitrate, Nickel Nitrate, Lead Nitrate, and Cobalt Nitrate with Group B
2: Reactions of all solutions
Key
A
E
Nitric Acid
1
Sodium Carbonate
5
EDTA
9
B
Copper
Nitrate
Nickel Nitrate
F
Silver Nitrate
2
Sodium Sulfate
6
10
C
Lead Nitrate
G
3
Cobalt Nitrate
H
Ammonium
Hydroxide
Sodium Chloride
7
D
Aluminum
Nitrate
Iron Nitrate
Sodium
Iodide
Sodium
Thiocyanate
Sodium
Chromate
4
8
11
12
Sodium
Dichromate
Sodium
Hydroxide
Demineralized
Water
Chemicals
before reaction
Double Replacement
Double Displacement: also called a metathesis reaction is when the anions and cations of two
different molecules switch places, forming two entirely different compounds. These reactions
are in the general form:
AB + CD > AD + CB
Precipitation reactions are one type of double replacement reaction.
Sodium Carbonate
Elements
Copper Nitrate
Nickel Nitrate
Lead Nitrate
Cobalt Nitrate
Nitric Acid
Silver Nitrate
Aluminum Nitrate
Iron Nitrate
Formula
Cu(NO3)2 + Na2CO3 --> CuCO3 + 2NaNO3
Ni(NO2)2 + Na2CO3 --> NiCO3 + 2NaNO2
Pb(NO3)2 + Na2CO3 --> PbCO3 + 2NaNO3
Co(NO3)2 + Na2CO3 --> CoCO3 + 2NaNO3
No reaction
AgNO3 + Na2CO3 --> Ag2CO3 + 2NaNO3
Al(NO3)3 + Na2CO3 --> AlCO3 + Na2(NO3)3
Fe(NO3)3 + Na2CO3 --> FeCO3 + Na2(NO3)3
Sodium Chloride
Elements
Copper Nitrate
Nickel Nitrate
Lead Nitrate
Cobalt Nitrate
Nitric Acid
Silver Nitrate
Aluminum Nitrate
Iron Nitrate
Formula
No reaction
No reaction
No reaction
No reaction
No reaction
AgNO3 + 2NaCl --> AgCl + 2NaNO3
No reaction
No reaction
Evaluation
The aim of this experiment was to find out the reasons why Copper Nitrate shows
visible reaction when mixed with Sodium Carbonate but no reaction when mixed with Sodium
chloride. According to the experiment, thick precipitate formed when Cooper Nitrate reacted
with Sodium Carbonate, but there was no reaction between copper Nitrate and Sodium
Chloride.
The chemical formula of copper (II) nitrate is Cu(NO3)2. It is commonly referred to
simply as copper nitrate. Anhydrous from of copper nitrate is blue, crystalline solid. The
hydrated forms of copper nitrate like we used for this lab also have blue color. Also, it’s
hygroscopic. It hydrates very soluble in ethanol and water.
Sodium Carbonate, Na2CO3, is also known for washing soda. It is a sodium salt of
carbonic acid. It is a white solid. It is insoluble in alcohol and ethanol but soluble in water.
Sodium carbonate is used in manufacturing glass. Also, it is used as an electrolyte in chemistry.
Besides, it is used as a water softener during laundry. It is very effective at removing stains
such as oil, grease and alcohol.
Sodium Chloride, 2NaCl, is also known as common salt. It consists most salinity of ocean
and extracellular fluid of many organisms. Since it is edible, it is often used as a condiment
and food preservative. It pulls water out of bacteria through osmotic pressure. This prevents
the bacteria to reproduce and spoil the food. It is colorless (or white) crystalline solid. It is
odorless, and soluble in glycerol, ethylene glycol, and formic acid. But, it is insoluble in HCL.
Copper and chlorine do not react rapidly at room temperature. On the other hand,
they react strongly if the copper is heated. This may explain why copper nitrate didn’t react
with sodium chloride.
There were also many mistakes that might have affected the experiment. First of all,
the amount of the solutions that we put was not consistent all the time. Sometimes, we poured
too little amount of solutions. That might caused mistakes because we would think there had no
reaction although they actually had reacted. In addition, I think we observed the reaction
enough. In other words, we observed and recorded the reaction right after we poured the
solution. However, some reacted quite slowly, and some kept reacting. There could be some
reactions that we didn’t catch. Lastly, we didn’t really observe the odor. This was very big
mistake because some solutions would have no reaction but only odor. Therefore, if I’m doing
this experiment again next time, I would be trying to be exact, and observe more carefully to
improve this lab.