1. Write balanced net ionic equations for the following reactions: a) The precipitation of the chloride of Hg22+ in Step 1. b) The formation of a yellow precipitate in Step 3. c) The formation of a black precipitate in Step 4. d) The reaction that occurs in Step 5. Step 3: Identification of Pb2+. To the solution test tube saved from Step 2, add one drop of 6 M acetic acid and a few drops of 0.1 M K2CrO4. If Pb2+ is present, a bright yellowish-orange precipitate of PbCrO4 will form.
1. Write balanced net ionic equations for the following reactions: a) The precipitation of the chloride of Hg22+ in Step 1. b) The formation of a yellow precipitate in Step 3. c) The formation of a black precipitate in Step 4. d) The reaction that occurs in Step 5. Step 3: Identification of Pb2+. To the solution test tube saved from Step 2, add one drop of 6 M acetic acid and a few drops of 0.1 M K2CrO4. If Pb2+ is present, a bright yellowish-orange precipitate of PbCrO4 will form.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.10QE: Draw the flow diagram for a calculation that illustrates how to use a titration to determine the...
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Balanced net ionic equation of b)
Transcribed Image Text:1. Write balanced net ionic equations for the following reactions:
a) The precipitation of the chloride of Hg22+ in Step 1.
b) The formation of a yellow precipitate in Step 3.
c) The formation of a black precipitate in Step 4.
d) The reaction that occurs in Step 5.
Transcribed Image Text:Step 3: Identification of Pb2+.
To the solution test tube saved from Step 2, add one drop of 6 M acetic acid and a few drops of
0.1 M K2CrO4. If Pb2+ is present, a bright yellowish-orange precipitate of PbCrO4 will form.
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