Lab Experiment: Ionic Reactions
Edward Dickson CHE101 DS-01 Experiment Date 7/21/2013 Report Submitted 7/21/2013
Title: Experiment #8: Ionic Reactions
Purpose: In this lab we will work with aqueous solutions of ionic substances and determine if they are soluble. If the solution appears milky than it is known as a precipitate reaction, meaning it is soluble, and that the ions separated and became surrounded by water. Precipitates in this experiment are electrically uncharged. To identify which compounds are soluble or insoluble we can check the chart in the textbook containing solubility rules and tables. The goal of the experiment is to study and observe the nature of ionic reactions.
Procedures:
Perform the following actions in the 96-well plate.
Place 2 drops of cobalt (II) nitrate solution into seven of the A row wells.
Place 2 drops of copper (II) nitrate into seven of the B wells.
Place 2 drops of iron (III) nitrate into seven of the C wells.
Place 2 drops of barium nitrate into seven of the D wells.
Place 2 drops of nickel (II) nitrate into seven of the E wells.
7. Place 2 drops of sodium phosphate solution into five vertical wells under column number 1.
Place 2 drops of sodium iodide solution into five vertical wells under 2.
Place 2 drops of sodium sulfate solution into five vertical wells under 3.
Place 2 drops of sodium chloride solution into five vertical wells under 4.
Place 2 drops of sodium bicarbonate solution into five vertical wells under 5.
Place 2 drops ofcarbonate solution into five vertical wells under 6.
Place 2 drops of sodium hydroxide solution into five vertical wells under 7. Record all results in the chart.
Observations:
|Negative Ion (Anion) |Positive Ions (Cations) |
|all negative ions are SOLUBLE with |Sodium phosphate |
|all negative ions are INSOLUBLE with |sodium sulfate |
|all negative
Title: Experiment #8: Ionic Reactions
Purpose: In this lab we will work with aqueous solutions of ionic substances and determine if they are soluble. If the solution appears milky than it is known as a precipitate reaction, meaning it is soluble, and that the ions separated and became surrounded by water. Precipitates in this experiment are electrically uncharged. To identify which compounds are soluble or insoluble we can check the chart in the textbook containing solubility rules and tables. The goal of the experiment is to study and observe the nature of ionic reactions.
Procedures:
Perform the following actions in the 96-well plate.
Place 2 drops of cobalt (II) nitrate solution into seven of the A row wells.
Place 2 drops of copper (II) nitrate into seven of the B wells.
Place 2 drops of iron (III) nitrate into seven of the C wells.
Place 2 drops of barium nitrate into seven of the D wells.
Place 2 drops of nickel (II) nitrate into seven of the E wells.
7. Place 2 drops of sodium phosphate solution into five vertical wells under column number 1.
Place 2 drops of sodium iodide solution into five vertical wells under 2.
Place 2 drops of sodium sulfate solution into five vertical wells under 3.
Place 2 drops of sodium chloride solution into five vertical wells under 4.
Place 2 drops of sodium bicarbonate solution into five vertical wells under 5.
Place 2 drops ofcarbonate solution into five vertical wells under 6.
Place 2 drops of sodium hydroxide solution into five vertical wells under 7. Record all results in the chart.
Observations:
|Negative Ion (Anion) |Positive Ions (Cations) |
|all negative ions are SOLUBLE with |Sodium phosphate |
|all negative ions are INSOLUBLE with |sodium sulfate |
|all negative