Zinc and HCl: Interaction between Zinc and HCl caused the once clear HCl to become white in color. Visible bubble can be observed around the Zinc metal.…
As observed there was a color change and solid precipitate noted, of which the calcium and carbonate ions. The sodium and chlorine are cancelled, as spectator…
Sodium chloride, sodium iodide, and sodium sulfates generally do not form precipitates. One exception in our results with all three of these was when they were each combined with Fe(NO3)3 (iron nitrate) in which all three yielded brown precipitates.…
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.…
Determine whether an ionic double replacement reaction has occurred.If I place different amounts of ionic solutions in a well plate, then I will be able to determine which of the solutions has had an ionic double reaction placement because I will use the solubility rules to decide which product produced the solid precipitate.Place five drops of silver nitrate into well A1 through A4. Place five drops of Iron (III) Nitrate into rows B1 through B4. Place 5 drops of copper (III) nitrate into rows C1 through C4. Now you will place four different ionic solutions in each column 1 through 4. Place five drops of Potassium Iodide in column 1A, 1B and 1C. Place five drops of sodium sulfate in column 2A, 2B, and 2C. Place five drops of sodium hydroxide in column 3A, 3B, and 3C. Place five drops of sodium chloride in column 4A, 4B, and 4C. Record the color of a precipitate that has formed in the data table and “NR” if no precipitate has formed showing no sign of a reaction.Add a little water to each well and turn the well plate over on a paper towel. Throw the towel away and clean the plate. 1. H2CO3. 2. CaCl2 (aq), H2CO3 (s). 3. Sodium Carbonate aqueous plus hydrogen Chloride aqueous yields Sodium Chloride plus Hydrogen Carbonate. 4. Well…
After completing this experiment several of the chemicals just simply changed colors. The main colors shown were blue, yellow, pink, green, and a brownish black. A few of the reactants did not change to a different color at all, but did show little signs of bubbles at the surface.…
18. Solution Both NaCl and NaBr give white and pale yellow ppts of AgCl and AgBr respectively on reaction with AgNO3.…
After the addition of silver nitrate, a dirty white solution with brown layer on top was produced.…
G.|KI + Pb(NO3)2|A8|A thick bright yellow gradually took over the mixture. Under white paper the mixture appears thick almost yolk like. Under black paper you can see the color pop from the rest of the mixtures. Became a precipitate. |…
J.|NaOH + AgNO3||Turns a dark brown and separates into small strands of brown liquid within the clear liquid. Heterogeneous|…
In this experiment, the student studied the composition of materials in a setting where the indications of chemical changes were safely observed. The changes observed consisted of bubble formation, colors, viscosity, and precipitate formation.…
Purpose: The purpose of this lab is to investigate the reliability of the activity series of metals by testing in solution, confirming if the activity series was correct with its predictions.…
3. When salicylic acid is added to a neutral solution such as iron chloride it turns intense pink colour. ( presence of a phenol- OH attached to a benzene ring )…
A double replacement reaction is a chemical reaction that usually takes place between two aqueous ionic…
FeCl2 was a green, pebbly powder. The DMSO was clear and colorless. When combined in the Erlenmeyer flask, the solution was clear and yellow. After heating and cooling in the ice bath, the solution resembled tea; it was dark brown and clear. After adding the solution dropwise into the round bottom flask, the solution turned a dark black color. Once the flask was washed with water and the contents poured into a beaker, the solution had two layers; the top thin layer was orange and oil-like, and the bottom was a dark green-black solution. After Buchner filtration, the filtrate was an aquamarine clear solution, while the residue was an orange-brown mat with a distinct smell.…