Chemistry, 17.04.2020 18:21 alexussaniyah
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?
a. The unknown solution definitely has Ag+ present.
b. The unknown solution could have Ag+ present, or Hg2^2+ present, or BOTH.
c. The unknown solution definitely has Hg2^2+ present.
d. The Unknown Solution definitely has Pb^2+ present.
Answers: 1
Chemistry, 22.06.2019 23:30
The density of the solid phase of a substance is 0.90 g/cm3 and the density of the liquid phase is 1.0 g/cm3. a large increase in pressure will a. lower the freezing point b. raise the freezing point c. lower the boiling point d. raise the triple point e. lower the triple point
Answers: 1
Chemistry, 23.06.2019 11:20
Try to reduce the amount of leftover ingredients by changing the amount of one, two, or all three starting ingredients. show your stoichiometric calculations below. water 946.36 g sugar 196.86 g lemon juice193.37 g
Answers: 2
Chemistry, 23.06.2019 19:30
What are the relative strengths of intermolecular forces compared to the forces between ions in a salt or the forces between metal atoms in a metallic bond?
Answers: 1
The procedure for testing your unknown solution in this week's lab is identical to the procedure whi...
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