Chapter 36
Chemical Principles in the Laboratory · 2 exercises
Problem 2
Write balanced net ionic equations for the following reactions: a. The precipitation of the chloride of \(\mathrm{Hg}_{2}^{2+}\) b. The dissolving of \(\mathrm{PbCl}_{2}\) in hot water. c. The dissolving of AgCl in aqueous ammonia.
6 step solution
Problem 4
A solution may contain \(\mathrm{Ag}^{+}, \mathrm{Pb}^{2+},\) and \(\mathrm{Hg}_{2}^{2+} .\) A white precipitate forms on addition of \(6 \mathrm{M}\) HCl. The precipitate is insoluble in hot water. The residue turns black on addition of ammonia. Which of the ions are present, which are absent, and which remain undetermined? State your reasoning. Note: On paper unknowns such as this one, confirmatory tests are usually not included. Present _____ Absent _____ In doubt _____
5 step solution