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 | Color| A1| |
Learning Target 2: The student will be able to say I have completed and defended balanced equations (including phase labels) by applying the laws of conservation of mass and constant composition.
Pre Lab Questions: