Lab 8 Ionic Reactions

Topics: Sodium chloride, Solubility, Sodium hydroxide Pages: 8 (1245 words) Published: July 16, 2014
Ocean County College
Department of Chemistry
Ionic Reactions
Submitted by:

Date Submitted: July 10, 2014
Date Performed: July 8 2014
Lab Section: Chem 181-DL2
Course Instructor: Amal Bassa

Background
Aqueous solutions of ionic substances will be experimented with in this Ionic Reactions lab. Aqueous solutions are solutions that water is solvent. After ionic substances dissolve in water, ions separate and become surrounded by water molecules. When these ion separate, its called dissociation.

Purpose
The purpose of this experiment is to study ionic reactions, to be able to write balanced equations, and to be able to write net ionic equations for precipitation reactions.

Procedure
First, all reactions will be completed in the 96-well plate. Put two drops of cobalt (II) nitrate solution into seven of the A row wells. Put two drops of copper (II) nitrate into seven of the B wells. Put two drops of iron (III) nitrate into seven of the C wells. Put two drops of barium nitrate into seven of the D wells. Put two drops of nickel (II) nitrate into seven of the E wells. For the second part, when performing the following, never touch the tip of the pipette to the solution already in the well. Now, put two drops of sodium phosphate solution into five vertical wells under column number one. Put two drops of sodium iodide solution into five vertical wells under two. Put two drops of sodium sulfate solution into five vertical wells under three. Put two drops of sodium chloride solution into five vertical wells under four. Put two drops of sodium bicarbonate solution into five vertical wells under five. Put two drops of sodium carbonate solution into five vertical wells under six. Finally, put two drops of sodium hydroxide solution into five vertical wells under seven. When the observations have been documented, wash the 24-well plate and the 96-well plate under tap water until all leftovers of chemicals have disappeared. Use a cotton swab to remove immovable precipitates. If the precipitates are allowed to dry they are much harder to remove. Get rid of any unused material by flushing them down the sink with a lot of water and toss the empty pipettes in the trash.

Observations and Data
Co(NO3)2
+
Na3PO4

Precipitate

Purple
Co(NO3)2
+ NaI
NK
Co(NO3)2
+ Na2SO4
NK
Co(NO3)2
+ NaCl

NK
Co(NO3)2
+NaHCO3
Light Precipitate
Pink
Co(NO3)2
+Na2CO3
Precipitate Pink
Co(NO3)2
+NaOH
Precipitate

Dark Green
Cu(NO3)2
+
Na3PO4
Precipitate Green
Cu(NO3)2
+ NaI
Precipitate Yellow
Cu(NO3)2
+ Na2SO4
NK
Cu(NO3)2
+ NaCl
NK
Cu(NO3)2
+NaHCO3
Light Precipitate Green

Cu(NO3)2
+Na2CO3
Precipitate Green
Cu(NO3)2
+NaOH
Precipitate

Blue

Fe(NO3)3
+
Na3PO4
Precipitate Yellow
Fe(NO3)3
+ NaI
Gold
Fe(NO3)3
+ Na2SO4
NK
Fe(NO3)3
+ NaCl
NK
Fe(NO3)3
+NaHCO3
Yellow
Fe(NO3)3
+Na2CO3
Precipitate Yellow
Fe(NO3)3
+NaOH
Precipitate

Yellow
Ba(NO3)2
+
Na3PO4
Precipitate White
Ba(NO3)2
+ NaI
NK
Ba(NO3)2
+ Na2SO4
Precipitate White
Ba(NO3)2
+ NaCl
NK
Ba(NO3)2
+NaHCO3
Light Precipitate
White
Ba(NO3)2
+Na2CO3
Precipitate
White
Ba(NO3)2
+NaOH
Light
Precipitate
Ni(NO3)2
+
Na3PO4
Precipitate Tan
Ni(NO3)2
+ NaI
NK
Ni(NO3)2
+ Na2SO4
NK
Ni(NO3)2
+ NaCl
NK
Ni(NO3)2
+NaHCO3
Light precipitate Grey
Ni(NO3)2
+Na2CO3
Light Precipitate Tan
Ni(NO3)2
+NaOH
Light Precipitate Tan
Questions
A. Compare your results with the solubility rules and/or solubility table in your chemistry text.

B. Do your results agree with your expectations from the solubility rules/table? Yes, I feel like they were similar to the rules on the table in the chemistry text.

C. Which anions generally form precipitates? What are exceptions? Many salts of carbonate: CO 2-, phosphate: PO 3-, oxalate: C2O4 2-, chromate, CrO4 2-, sulfide: S 2-, and the majority of metal hydroxides and oxides. Exceptions include alkali metal hydroxides and...
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