1. For Part 1, describe the changes in the colors of the well, if any, as you go from well 1 to well 9—that is, as you go from the well with the least copper(II) nitrate to the well with the most co

1. For Part 1, describe the changes in the colors of the well, if any, as you go from well 1 to well 9—that is, as you go from the well with the least copper(II) nitrate to the well with the most copper(II) nitrate. Which wells had the most distinct precipitate?

For Part 2, describe the changes in the colors of the well, if any, as you go from well 1 to well 9—that is, as you go from the well with the least iron(II) sulfate to the well with the most iron(II) sulfate.

For Part 3, describe the changes in the colors of the well, if any, as you go from well 1 to well 9—that is, as you go from the well with the least iron(III) nitrate to the well with the most iron(III) nitrate.

2. Below are the balanced equations for the reactions in Parts 1–3. Review the results of your experiments and look closely over the mole ratios of the chemical reactions. Do your experiments reflect the stoichiometric, molar amounts indicated by the reactions? Discuss this using the evidence from your experiments.

Cu(NO3)2 (aq) + 2NaOH (aq)  Cu(OH)2 (s) + 2NaNO3 (aq) Note: Cu(OH)2 is a blue precipitate.

FeSO4 (aq) + 2NaOH (aq)  Fe(OH)2 (s) + Na2SO4 (aq) Note: Fe(OH)2 is a dark green precipitate.

Fe(NO3)3 (aq) + 3NaOH (aq)  Fe(OH)3 (s) + 3NaNO3 (aq) Note: Fe(OH)3 is a red-orange precipitate.