Ferricyanide Reaction Lab

Introduction
For this lab, a number of reactions were performed to aid in the identification of a set of cations. This process was performed to show the effects various chemicals have on the given set of cations. The method through which this experiment was performed included mixing two reactants, a cation and a chemical compound, then examining whether or not a precipitate was created by the mixture. If a precipitate did form, the mixture was then centrifuged to solidify whatever insoluble material was created. After decanting, washing and re-centrifuging the solution, the now semi-pure solid was then submerged in Sodium Hydroxide, while once again recording the appearance of the solution. Many of the methods used in this lab would be most

Yellow hue, but no actual reaction between the Aluminum and Ferricyanide
Slight yellow hue from the Ferricyanide but once again no actual reaction
Blood Red precipitate was formed by combining Cobalt and Ferricyanide
Yellow sludgy precipitate was formed
Mustard-colored cloud of precipitate material
PO43-
White cloudy precipitate was formed in solution
White precipitate that was dissolved from the addition of Water
Dark Purple precipitate was formed by combing Phosphate and Cobalt
Thin blue cloud of mineral like material
White precipitate
OH-
White precipitate was dissolved by the Hydroxide
N/A
Dark Blue precipitate that faded back to the original Pink the Cobalt solution had prior to mixing
Cloudy blue precipitate
Zinc-Hydron precipitate was dissolved by the addition of Sodium Hydroxide
NH3 (NH4OH)
N/A
N/A
The precipitate was barely affected by the Ammonia and remained solid
Precipitate dissolved, leaving a blue solution
N/A
H+
N/A
N/A
The solid was dissolved and the mixture reverted back to the Cobalt’s original Pink hue
The precipitate once again dissolved, leaving a green solution
N/A
The table above shows the numerous cations and chemicals experimented upon and the visual observations each reaction yielded

Data Analysis &

I would then add a fair amount of Sodium Triphosphate. If the white precipitate and only the white precipitate remains, I could be sure the solution did in fact only contain Ca2+ Ions.

Scenario 2: For scenario two, I would add some Potassium Ferrocyanide to the solution supposedly containing Zn2+ and Ca2+ ions. If the solution yielded a yellow precipitate, Zinc is present. If only a white precipitate remained, Ca2+ is present. If there’s combination of yellow and white precipitate material, then both are present.
Scenario 3: For this scenario involving a solution supposedly containing Al3 and Co2+, I would add several drops of Ammonia. If the solution produces a dark precipitate, then cobalt is present. No precipitate would mean that Al3+ was present and a lightly colored precipitate means there is a mix of both.