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Ion Tests Laboratory Write-up

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Introduction

Nicole Calo Chemistry Ms. Semkin Oct. 15, 2008 Ion Tests Data: Data Table 1: Reactions of certain anions contained in aqueous solutions when specific compound solutions (used as indicators) are added. Anion Aqueous Solution Indicator Solution Added Result Carbonate Sodium Carbonate Dilute Nitric Acid The liquid effervesces since gas (Carbon Dioxide) is released. Barium Chloride White precipitate is formed. Sodium Hydroxide * Silver Nitrate * Potassium Thiocyanate * Sulfate Sodium Sulfate Barium Chloride White cloud-like precipitate is formed. Dilute Nitric Acid * Sodium Hydroxide * Silver Nitrate * Potassium Thoicyanate * Chloride Sodium Chloride Silver Nitrate White and milky precipitate is formed. After left in sunlight, color darkens to lilac. Barium Chloride No visible reaction. Sodium Hydroxide * Dilute Nitric Acid * Potassium Thiocyanate * Iodide Potassium Iodide Silver Nitrate Color change to milky light yellow. Milky precipitate in suspension is formed. Barium Chloride * Sodium Hydroxide * Dilute Nitric Acid * Potassium Thiocyante * Bromide Sodium Bromide Silver Nitrate Cloudy white precipitate is formed. Barium Chloride * Sodium Hydroxide * Dilute Nitric Acid * Potassium Thiocyanate * Data Table 2: Reactions of certain cations contained in aqueous solutions when specific compound solutions (used as indicators) are added. Cation Aqueous Solution Indicator Solution Added Result Aluminum Aluminum Hydroxide Sodium Hydroxide Cloudy rosy white precipitate is formed. Barium Chloride * Silver Nitrate * Dilute Nitric Acid * Potassium Thiocyanate * Zinc Zinc Sulfate Sodium Hydroxide Cloudy white swirling precipitate is formed. ...read more.

Middle

The precipitates formed are sodium nitrate and silver chloride. Iodide - When aqueous potassium iodide reacts with aqueous silver nitrate a color change to milky yellow takes place and milky precipitate is formed. Potassium, iodide, silver, and nitrate ions are present in this reaction. The precipitates formed are potassium nitrate and silver iodide. Bromide - When aqueous sodium bromide reacts with aqueous silver nitrate a milky white precipitate is formed. Sodium, bromine, silver, and nitrate are the ions present in this reaction. The precipitate is silver bromide. Cations Aluminum - When aqueous aluminum hydroxide reacts with aqueous sodium hydroxide a cloudy rosy white precipitate is formed. Sulphate, sodium, and hydroxide ions are present in this reaction. The precipitate formed is iron hydroxide. Zinc - When aqueous zinc sulfate reacts with aqueous sodium hydroxide a white precipitate is formed. Iron, sulphate, sodium, and hydroxide are the ions present in this reaction. The precipitate formed is zinc hydroxide. Iron(II) - When aqueous iron sulphate reacts with aqueous sodium hydroxide a color change to mossy green occurs while the heavy precipitate formed gathers at the bottom. Iron, sulphate, sodium, and hydroxide are the ions present in this reaction. The precipitate formed is iron hydroxide. Iron(III) - When aqueous iron chloride reacts with aqueous potassium thiocyanate a color change to orange takes place. Iron, chlorine, sodium, and hydroxide are the ions present in this reaction. The precipitate formed is iron hydroxide. Iron(III) ...read more.

Conclusion

Secondly, it would be more convenient if the solutions were placed on one or two tables near each other rather several meters away from each other which causes the hassle of having to walk back and forth the room, maneuvering through desks, to do a new test each time. Relatively, part of the inconvenience was having to pour out the content of the single test tube over and over for it to be used for the next test and having to go back and forth the room to each time. It would have been better if a rack of test tubes was supplied so that the experimenter wouldn't have to keep pouring out each mixture to perform a new test. Aside from that, the time necessary in performing this experiment because of the way it had been set up is long. However, the time available was short and so it was not possible for the experiment to be carried out completely, (as is seen in the data gathering section of this lab report). Yet most of the shortcomings this experiment is understandably due to the fact that there are many students in the class - therefore crowding up would take place if all the solutions were place on one table, and there are possibly not that many test tubes available for each student to have a set of, and the class period is only for a set amount of time; we cannot extend it freely to accommodate our purposes. ...read more.

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