Question

QUESTION 1 The procedure for testing your unknown solution in this week's lab is identical to the procedure which you conducted in Week 1. The only difference is, of course, your Unknown Solution may or may not contain all of the ions which you tested for in Week 1. With that being said, please consider the following scenario: You enter the lab and obtain an unknown Solution from the Stockroom. You begin testing the solution through the steps outlined in the flowchart on p. 9 of the Exp 22 document. You first add HCl, and centrifuge your mixture. You observe the formation of a white precipitate in the bottom of the test tube. After pouring off the supernatant liquid, you add hot water to the white precipitate. Upon addition of the hot water, you still have some white precipitate in the bottom of the test tube. Which of the following is a correct conclusion to draw at this point? (Choose only one answer.) The unknown solution definitely has Ag* present. The unknown solution could have Agt present, or Hg22 present, or BOTH. The unknown solution definitely has Hg2+ present. The Unknown Solution definitely has Pb2+ present. QUESTION

Answer 1

solution after testing with dil. Hle gives white precipitation & Group I cation present Ag+, Pyth, Hg, 27 Agce , Pbly, Hgalla (white ppt) After dissolving the ppt in hot water, some white ppt is still left. Pbly is soluble in hot water in appreciable amount. The solubility of bblle increases abruptly with increase in temperature & whereas Age and Hogall are sparingly soluble in hot water te & The unknown solution could have Ag+ , Hg, 7 present or both.