You have the following solutions available in the lab: NH4Cl, NaOH, HCl, and CuSO4. 1. Predict which pair of compounds will produce a precipitate. Use the solubility rules listed above. 2. Test your prediction by combining about 1 mL each of the two solutions in a clean and dry test tube. Record the results of your test below and write the net ionic equation for the reaction.
1. Group 1 metal compounds (also called alkali metal compounds), acetates, nitrates, and ammonium compounds are all soluble.
2. Hydroxides of alkali metals and NH4+1, Ca+2, Sr+2, and Ba+2 are soluble. All others are insoluble.
3. All halides (chlorides etc.) are soluble except for those containing Ag+1, Pb+2, and Hg2+2.
4. Most sulfates are soluble, except for BaSO4, SrSO4, Ag2SO4, PbSO4, and CaSO4.
5. Most phosphates, carbonates, chromates and sulfides are insoluble (except those of the Group 1 metals and ammonium ion).6. In addition, all acids (compounds that form an ionized H+, HCl, H2SO4, HI, etc.) are soluble!You have the following solutions available in the lab: NH4Cl, NaOH, HCl, and CuSO4.
1. Predict which pair of compounds will produce a precipitate. Use the solubility rules listed above.
2. Test your prediction by combining about 1 mL each of the two solutions in a clean and dry test tube. Record the results of your test below and write the net ionic equation for the reaction.
3. Compounds tested:
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