|?40 Late Nite Labs Late Nite Labs × SilverGroup.pdf CHE101-LabAssignment,Mi + ?

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|?40 Late Nite Labs Late Nite Labs × SilverGroup.pdf CHE101-LabAssignment,Mi + ? a https://labs.latenitelabs.com/api/assessment/shortAnswer/307593/102440 Formats- Paragraph ? Arial NOTES decant all material left little bit of yellow in bottom 1. Why do you need hot water to dissolve the lead chloride? 2. Suppose you had to identify the group I cation(s) in a third unknown sample, Given the data in the table below, what cations are present in the powder? Test # | Reaction reaction with HCl precipitate from the HCI reactionhot water precipitate from test 2 ammonia supernatant from test 2K2CrO supernatant from test 3 HNO3 Observations white precipitate formed white precipitate still in solution black precipitate formed ellow precipitate formed no reaction DIV> OL LI 345 WORDS POWERED BY TINYMCE SUBMIT FOR GRADING SAVE AND FINISH LATER Discard changes Back to assignments 5:50 PM O Type here to search 7/6/2018 21

Explanation / Answer

1. Lead chloride is insoluble in water at ambient temperature but is soluble in hot water. For the reason, it is dissolved in hot water.

2. Reaction with HCl: white precipitate is obtained which indicates that Ag+, Pb+2 or Hg2+2 may be present

Precipitate from HCl reaction + hot water : white precipitate still in solution - May contain Ag+ (as AgCl) or Hg2+2 (as Hg2Cl2)

precipitate from 2 + NH3: black precipitate - It is Hg(NH2)Cl: Hg2+2 is confirmed

supernatant from test 2 + K2CrO4 : yellow precipitate - it is PbCrO4 : Pb+2 is confirmed

Supernatant from test 3 + HNO3 : no reaction: Ag+ is absent

The cations present in the sample are: Hg2+2 and Pb+2

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