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
Transcript
Wendy Kim 1ALab Science 9
Ms. NakaiDouble Replacement Reaction
ProblemWhy does Copper (II) Nitrate show visible reactions with Sodium Carbonate but not with Sodium Chloride?
HypothesisIf 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 MethodEach 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:Chemicals0.1M solutions of the following:
Group ACopper (II) NitrateNickel (II) NitrateLead (II) NitrateCobalt (II) NitrateNitric AcidSilver NitrateAluminum NitrateIron (III) Nitrate
Group BSodium CarbonateSodium SulfateAmmonium HydroxideSodium ChlorideEDTASodium IodideSodium ThiocyanateSodium ChromateSodium DichromateSodium HydroxideDemineralized Water
*Highlighted chemicals are the ones that I used for my hypothesis.Hardware96-well mirco platePipettes
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
Sodium Iodide
Sodium Thiocyanate
Sodium Chromate
Sodium Dichromate
Sodium Hydroxide
Demineralized Water
Copper Nitrate
Turns green, yellow, forms orange precipitate
Turns green
Turns dark yellow, precipitate formed
Turns dark yellow, slight precipitate
Precipitate formed
No reaction
Nickel Nitrate
No reaction No reaction Turns yellow-green
Turns dark yellow
No reaction
No reaction
Lead Nitrate
Turns bright yellow, forms precipitate
No reaction Turns bright yellow, precipitate formed
Turns bright yellow, precipitate formed
Precipitate formed
No reaction
Cobalt Nitrate
No reaction No reaction Turns orange-brown
Turns orange
Turns blue, precipitat
No reaction
Sodium Carbonate
Sodium Sulfate
Ammonium Hydroxide
Sodium Chloride
EDTA
Copper Nitrate
Thick precipitate formed
Turns clear Slight precipitate formed
No reaction Turns bluer
Nickel Nitrate
Thick precipitate formed
No reaction No reaction No reaction Turns blue
Lead Nitrate Thick precipitate formed
Thick precipitate formed
Turns blue No reaction No reaction
Cobalt Nitrate
Thick precipitate formed
No reaction Turns blue, precipitate formed
No reaction No reaction
Nitric Acid No reaction No reaction No reaction No reaction No reactionSilver Nitrate Thick
precipitate formed (white)
No reaction Slight precipitate (white)
Turns opaque white, precipitate
Precipitate formed
Aluminum Nitrate
Precipitate formed (white)
No reaction Slight precipitate formed
No reaction No reaction
Iron Nitrate Precipitate formed (turns darker)
No reaction Precipitate formed, turns darker
No reaction No reaction
e formedNitric Acid
No reaction No reaction Turns yellow
Turns yellow
No reaction
No reaction
Silver Nitrate
Forms pale-green precipitate
Precipitate formed
Turns dark red, precipitate formed
Turns dark red-brown, precipitate formed
Turns brown, precipitate formed
No reaction
Aluminum Nitrate
No reaction No reaction Turns yellow, precipitate formed
Turns yellow (no precipitate)
Slight precipitate formed
No reaction
Iron Nitrate
Turns darker Forms layer of dark, opaque red
Turns orange, precipitate formed
Turns orange-yellow, precipitate formed
Turns dark orange-yellow, precipitate
No reaction
Data Processing
1: Reactions of Copper Nitrate, Nickel Nitrate, Lead Nitrate, and Cobalt Nitrate with Group B
2: Reactions of all solutions
KeyA Copper
NitrateE Nitric Acid 1 Sodium
Carbonate5 EDTA 9 Sodium
DichromateB Nickel
NitrateF Silver Nitrate 2 Sodium
Sulfate6 Sodium
Iodide10 Sodium
HydroxideC Lead
NitrateG Aluminum
Nitrate3 Ammonium
Hydroxide7 Sodium
Thiocyanate
11 Demineralized Water
D Cobalt Nitrate
H Iron Nitrate 4 Sodium Chloride
8 Sodium Chromate
12 Chemicals before reaction
Double ReplacementDouble 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 + CBPrecipitation reactions are one type of double replacement reaction.
Iron Nitrate Fe(NO3)3 + Na2CO3 --> FeCO3 + Na2(NO3)3
Sodium ChlorideElements FormulaCopper Nitrate No reactionNickel Nitrate No reactionLead Nitrate No reactionCobalt Nitrate No reactionNitric Acid No reactionSilver Nitrate AgNO3 + 2NaCl --> AgCl + 2NaNO3Aluminum Nitrate
No reaction
Iron Nitrate No reaction
EvaluationThe 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.
