Solubility Lab Report

In part 1 the results of the solubility do not agree with the with rules of solubility most likely because we put too much solid in the test tubes and not enough water to dissolve it. They should have dissolved because the anything with nitrate should be soluble. With the pH, when the mixture where compared with the chart all of them except NaCl where a shade of blue which means that they have a pH of 8-14, depending on the darkness of the shade, meaning that they are a basic solution. When reacting with the HNO3 most of the solutions had a color change to acidic which the addition of only one drop, whereas with Na2Cl3 it bubbled over and changed color with the addition of 5 drops of HNO3. In our experiment we messed up the first time and forgot to divide the solutions in half, so we had to start all over, and make sure that we divided the solutions that second time. With addition of the last two acids in one half of the solutions all of them formed a precipitate because of the acid causing bubbles and creating the precipitate.
The limiting reagent it CuCl2 because it is the one that will run out first compared to the .009 moles of Na2Cl3, which it the excess reagent because it is a higher amount of moles compared to the .007 moles of the CuCl2.
The amount of excess reagent in grams that should remain in solution if the theoretical yield of CuCO3 is produced is:
1 mole of CuCl2  (63.55) +(2*35.45) =134.45
1mole of Na2Cl3  (22.99 *2) +(12.01) +(3*16) =105.99 (this is the excess