Chemistry Lab – Precipitate Patterns

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Chemistry Lab – Precipitate Patterns Purpose: To identify which anion will be used to form a precipitate with the most metal cations. Procedure: All materials were obtained A chart was made to compare anions and cations Drops of sodium carbonate solution were placed in each section of the wet plate Dilute solutions of calcium carbonate were dropped into the sodium carbonate and observations were recorded Step 4 was repeated for all other reacting solutions and observations were recorded Chemicals were placed into a waste beaker and disposed of Lab station was cleaned Observation List: Na2CO3 + Ca(NO3)2  CaCO3 + NaNO3 -Formation of a precipitate Na2CO3 + Cu(NO3)2  CuCO3 + NaNO3 -Formation of a precipitate Na2CO3 + Fe(NO3)2  FeCO3 + NaNO3 -Formation of a precipitate Na2CO3 + Mg(NO3)2  MgCO3 + NaNO3 -Formation of a precipitate Na2CO3 + Zn(NO3)2  ZnCO3 + NaNO3 -Formation of a precipitate Na2CO3 + NaSO4  Na2CO3 + Na2SO4 -Formation of a precipitate Na2SO4 +Cu(NO3)2  CuSO4 + NaNO3 -Formation of a precipitate Na2SO4 + Ca(NO3)2  CaSO4 + NaNO3 -Formation of a precipitate Analyse and Evaluate: The investigation could have been improved of beakers were used instead of wet plates. This way, it would have been easier to see the reactions taking place. The anion that could be used to precipitate the most metals cations was carbonate. Carbonate could be used to remove silver ions. This is because when carbonate reacts with a cation other the H+ and NH4+, it has a low solubility. Meaning it would form a precipitate with silver and the ions would be removed. Evidence that suggest nitrate compound are soluble is that they didn’t with most compounds, they remained aqueous. Also, there was never a formation of a precipitate when reacting with nitrate ions. Na2CO3 + Ca(NO3)2CaCO3 + NaNO3 Na2CO3 + Cu(NO3)2 CuCO3 +

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