Monster Mash Lab Report

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Lesson written by Carolina Sylvestri Experiment: Reaction Between Ions in Aqueous Solutions The Monster Mash Background: Ionic solids dissolve in water to form aqueous solutions which conduct electricity. These solutions contain both positive and negative ions in such numbers that their net electric charge is zero. In this experiment, you will mix various ionic solutions, two at a time, to determine which combinations form precipitates. Knowing which ions are present makes it possible to deduce which of the possible ion combinations are responsible for the precipitates. From your data table, it will then be possible to generate a solubility table. Advice and general procedure: You must follow the directions for the prelab, and you…show more content…
Set #3 0.1M Co(NO3)2, 0.2M KOH, 0.2M NaNO3, 0.5M NaOH, 0.1M FeCl3, 0.1M CoCl2 Set #4 0.5M NaOH, 0.1M NiCl2, 0.14M Ba(OH)2, 0.2M MgCl2, 0.2M MgSO4, 0.2M Na2SO4 Set #5 0.1M Sr(NO3)2, 0.1M BaCl2, 0.14M Al2(SO4)3, 0.2M K2CrO4, 0.05M AgNO3 Sample data table: |Set 1 | | |Ba(NO3)2 |BaCl2 |K2CrO4 |K2SO4 |KCl | |Ba(NO3)2 | | | | | | |BaCl2 | | | | | | |K2CrO4 | | | | | | |K2SO4 | | | | | | |KCl | | | | |…show more content…
For example, if you mix aqueous solutions of AgNO3 and NaCl, there are two new combinations of ions possible. The silver nitrate solution contains Ag+(aq) and NO3-(aq). The sodium chloride contains Na+(aq) and Cl-(aq). Possible new combinations of these ions are AgCl and NaNO3. Note: these formulas would have been written in the upper right hand corner of each box before beginning the lab. 2) Examine your data to see if you can justify eliminating some of the combinations listed as possible precipitates in this experiment. For example, NaCl was an aqueous product in Set 1-15. Therefore it could not precipitate in another box or set. 3) Write equations to indicate what you consider to have happened in each case in which there was precipitate formed. Use ions to represent the species in the reacting solutions, but for those products that were precipitates write a formula for the compound. Place (aq) after those species in solution and (s) after the precipitates. Be sure to write the equations so that both atoms and charge are conserved. For example: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) ( AgCl(s) + Na+(aq) + NO3-(aq) 4) Rewrite the equations, leaving out the ions not involved in the reaction (spectators). Such an equation, which shows only the predominant reacting species, is called a net ionic equation. Ag+(aq) + Cl-(aq) (

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