Group I CationsA1. Explain why litmus paper is used in step 4. Why is blue litmus paper used rather than redlitmus paper?litmus Paper is used in Step y because2. Several steps involve the use of reactive compounds. Based on your laboratoryexperience, identify these steps and indicate any appropriate precautions you needto take. Qualitative AnalysisStep 2. The solubility of lead is sufficiently high that at low lead concentrations, all of thein addition, the solubility of lead increases about threefold in hot water compared to room temperature water; thus, a significant amount of lead can be solubilized from the mixture of AgCl,H92CI2, and P6CI2 by treating the mixture with hot water. Therefore, centrifuging the resultingsolution leaves only a solution of lead (if lead is present).Step 3. The presence of lead can be confirmed or eliminated by the addition of chromate toform the bright yellow solid PbCrO. (Equation 8). You may recognize this color because leadchromate is often the pigment in the yellow paint used to paint yellow lines on highways.Equation (8)Pb2*(aq) + Cro?-(aq) PbCrO4(s) Ksp = 1.8 × 10-14Step 4. The addition of aqueous ammonia results in the formation of the complex ion[Ag(NH3)21*, solubilizing the silver, but also in the disproportionation of the Hg* (i.e., Hg2") intoHg° metal and Hg2*, which forms the solid H9NH,CI under these conditions (Equations 9, 10,and 11).Equation (9)Hg2*(aq) := Hg°(s) + Hg2*(aq)Equation (10)Hg2*(aq) + CI(aq) + 2 NH3(aq) = H9NH2CI(s) + NHẬ(aq)Equation (11)AgCl(s) + 2 NH3(aq) =2[Ag(NH3)2]*(aq) + CI¯(aq)Finally, to confirm the presence of silver, the addition of acid results in the protonation of theammonia to the ammonium cation, resulting in the reprecipitation of silver chloride (Equation 12).Equation (12)[Ag(NH3)2]*(aq) + 2 H*(aq) + CI"(aq)=AgCI(s) + 2[NH4J*(aq)

Litmus papers are used to detect whether the given solution is acidic or basic.

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1. Explain why litmus paper is used in step 4. Why is blue litmus paper used rather than red litmus paper?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
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CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42- should be used so that Ag2CrO4(s) just starts to form at the equivalence point? If a concentration of 0.0010 M CrO42- is used instead, at what concentration of Br- will Ag2CrO(s) just start to precipitate? Do you think this is likely to introduce significant error? The Ksp for Ag2CrO4(s) is 1.2x10-12.
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How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solving