Purpose - In the next step when the lead nitrate solution...

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Purpose: To be able to determine the formula for the ionic solid formed in the reaction and to write the chemical equation for the reaction. Procedure: Please see pgs. 27-34 of General Chemistry Laboratory Experiments, Volume1 by Judith Casey and Robert Taz, Hayden, McNeil, 2009-2010 Report Sheets: See attached papers. Data: Table 4.1 used to prepare solutions. Drops of Pb(NO3)2 Drops of KI Drops of Water Tube 1 12 4 32 Tube 2 12 6 30 Tube 3 12 12 24 Tube 4 12 24 12 Tube 5 12 36 0 Report Questions: See attached papers. Conclusion: Parts A and B of this lab were relatively straight forward in the sense that you were mixing chemicals together with either KI or Pb(NO3)2 to see if either anions or cations were present in the solution as well as if a precipitate formed. I found a reaction did occur when iodine reacted with H2O2. This tells me that an anion is present. Also, a reaction occurred when lead was mixed with H2S showing that a cation had been present.
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Unformatted text preview: In the next step when the lead nitrate solution was added to the potassium iodide solution a precipitate formed when either H2O2 or H2S were added. In part C, the goal was to determine the exact ratio of ions in a precipitate, which proved to be more difficult. My sources of error I think showed in this step because it was hard to make sure the medicine dropper was thoroughly clean before switching to a different chemical. Also there was probably some human error when I tried adding the exact amount of drops to each solution. Having said that I did get the formula of the precipitate to be PbI2. Test tube four seemed to contain the correct ratio, as a very minimal amount of precipitate had formed in the test tube. This makes the ratio of drops 1Pb: 2I. When adding drops in this ratio no ions are present in excess....
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Purpose - In the next step when the lead nitrate solution...

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