USA: +1 (725) 712-1730 
Sign in
just need help with the table, thanks!
4. Using the information in Sections 4.1 and 4.2, as well as the line of illustrated in question 2 above, predict the outcome when each cation reacts wi the four reagents used in the preliminary tests. Complete the reaction table below in your lab notebook prior to coming to the first week of this lab. During the Week 1 lab period, you will characterize the behavior of your four assigned cations with the reagents; the predictions you make now will belp you analyze the results you find during Week 1. One cation is done completely for you as an example; the reasoning behind each entry is given as a footnote. You do not need to provide a written explanation for your entries these are provided as an example of the thinking to be applied when completing this reaction grid. NaCI NazSO4 NaOH NH3 (aq) Cation Al3+ Ba2- Cu2 Feh Mn2 N2+ S 50, Footnote 2 Footnote 3 Footnote 4 Footnote I According to the solubility rules, all chlorides are soluble except silver and lead. Therefore a precipitate is ce (color, etc.)of the precipitate will be noted during the lab period. However, since silver nd chloride can form a soluble complex ion, AgCl, addition of excess chloride may actually dissolve the
Expert Answer
| Cation | NaCl | Na2SO4 | NaOH | NH3 (aq) |
| Al3+ | solid AlCl3 | solid Al2(SO4)3 | solid Al(OH)3 | precipitate [Al(OH)3 and NH4+] |
| Ba2+ | solid BaCl2 | solid BaSO4 | solid Ba(OH)2 | precipitate [Ba(OH)2] |
| Cu2+ | greenish solid CuCl2 | blue solid, CuSO4 | solid Cu(OH)2 | blue precipitate [Cu(OH)2]
excess NH3 gives dark blue complex |
| Fe3+ | solid FeCl3 | solid Fe2(SO4)3 | solid Fe(OH)3 | orange precipitate [Fe(OH)3] |
| Mn2+ | solid MnCl2 | solid MnSO4 | solid Mn(OH)2 | brownish precipitate Mn(H2O)4(OH)2 |
| Ni2+ | solid NiCl2 | solid NiSO4 | solid Ni(OH)2 | blue solution [Ni(NH3)6] |
