The purpose should include a majority of the topics and techniques covered in the experiment. The procedure section should cite the lab manual and include any changes made to the procedure during lab work. The procedure section should also include a step-by-step procedure on how you determined the identity of the unknown.

The data section should include a table for parts I and III listing the seven cations down the side and with five columns labeled: Initial Observation, OH^-, xs OH^-, NH₃, and Anion PPT. In the first column record initial observations, noting the color of each solution.  In the remaining sections describe the results upon mixing. The combinations that you did not mix in lab form no reaction. Be sure to include things such as colors and formulas of precipitates. DO NOT RECORD "NO CHANGE"; RECORD WHAT THE SOLUTION/MIXTURE LOOKS LIKE EVEN IF IT IS CLEAR AND COLORLESS. For the anion precipitation column indicate which anions form a precipitate and all other observations. All observations written in this table must match those made during lab and recorded in your lab notebook.

For part II make a table with the observations you recorded in lab after each step. For parts IV and V include all observations in a systematic fashion.

For part VI (the identity of the unknown) include observations made during each step you took in lab, along with the code and identity of the cation(s) and anion(s) in your unknown.

The calculation section for this experiment will include balanced net ionic equations. Write the balanced net ionic equation for each reaction from Part I. If you observed a precipitate re-dissolve in excess OH^-, write two separate balanced equations: The first showing the formation of the precipitate from the metal ions and the hydroxide ion; and the second with the precipitates and additional hydroxide ions as the reactants. NH₃ was also reacted with all the cations except Na⁺, If a precipitate formed and remained, a neutral hydroxide salt formed when the cation reaction with NH₃ and H₂O. If a precipitate was not observed or immediately re-dissolved, the cation reacted with NH₃ to form a complex ion. Formulas of any complex ions can be determined from the information provided in the background section to this experiment. ALSO write the balanced net ionic equations for the anion precipitation reactions you observed in Part III.

The conclusion section should include several detailed paragraphs which include the following information: A paragraph explaining how a stability series works, include how the observations you made specifically illustrate the stability series for silver ions (this is from part II). The identity of the ions in your unknown and how you reached these conclusions. This should include a discussion of the known reactions you did in parts I-V and how they compare to the unknown reactions. Be sure to include a description of both supporting and eliminating experiments that you conducted.  Finally include all possible errors found in this experiment.

Answer the following questions:

1. Which cation forms a 2-ligand complex with NH₃?


2. Which anion does not form a precipitate with lead?


3. Write the balanced equation for the dissociation of the compound in question 2 in water.