Experiment on Ionic Reactions
Data Table: Record your observations in the following table
Na3PO4 NaI Na2SO4 NaCl NaHCO3 Na2CO3 NaOH
Co(NO3)2 Precipitated a blue color NR NR NR Turned a milky purple color Precipitated a light purple color Precipitated a light blue color
Cu(NO3)2 Precipitated a light blue color Precipitated a dark amber color NR NR Precipitated a light blue color Precipitated a light green color Precipitated a light blue color
Fe(NO3)3 Precipitated a light milky yellow color Turned a dark black color NR NR Turned a light yellow-gold color Precipitated an black color Precipitated an yellow color
Ba(NO3)2 Precipitated a beige milky color NR Precipitated a yellow milky color NR Precipitated a beige milky color Precipitated a yellow milky color Precipitated a beige milky color
Ni(NO3)2 Precipited a very light blue color NR NR NR Precipitated a beige milky color Precipitated a very transparent yellowish color Precipitated a very light bluish color
Conclusion: The purpose of this experiment is to work with aqueous solutions of ionic substances. Aqueous solutions are those solutions in which water is the solvent. When ionic substances are dissolved in water, the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions, write balanced equations, and to write net ionic equations for precipitation reactions. Based on the solubility rules my results proved accurate. Just by looking at the solubility rules, my results were what I expected them to be. I found that sodium chloride did not react with any of the five substances and that the sodium sulfate only reacted with the barium nitrate. The sodium bicarbonate, sodium carbonate as well as the sodium hydroxide reacted with all five substances. This was expected because the solubility rules stated that these were all insoluble substances. I was careful to add exactly two drops of each into
Na3PO4 NaI Na2SO4 NaCl NaHCO3 Na2CO3 NaOH
Co(NO3)2 Precipitated a blue color NR NR NR Turned a milky purple color Precipitated a light purple color Precipitated a light blue color
Cu(NO3)2 Precipitated a light blue color Precipitated a dark amber color NR NR Precipitated a light blue color Precipitated a light green color Precipitated a light blue color
Fe(NO3)3 Precipitated a light milky yellow color Turned a dark black color NR NR Turned a light yellow-gold color Precipitated an black color Precipitated an yellow color
Ba(NO3)2 Precipitated a beige milky color NR Precipitated a yellow milky color NR Precipitated a beige milky color Precipitated a yellow milky color Precipitated a beige milky color
Ni(NO3)2 Precipited a very light blue color NR NR NR Precipitated a beige milky color Precipitated a very transparent yellowish color Precipitated a very light bluish color
Conclusion: The purpose of this experiment is to work with aqueous solutions of ionic substances. Aqueous solutions are those solutions in which water is the solvent. When ionic substances are dissolved in water, the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions, write balanced equations, and to write net ionic equations for precipitation reactions. Based on the solubility rules my results proved accurate. Just by looking at the solubility rules, my results were what I expected them to be. I found that sodium chloride did not react with any of the five substances and that the sodium sulfate only reacted with the barium nitrate. The sodium bicarbonate, sodium carbonate as well as the sodium hydroxide reacted with all five substances. This was expected because the solubility rules stated that these were all insoluble substances. I was careful to add exactly two drops of each into