The solubility of silver bromate, $\mathrm{AgBrO}_3$, in water is $0.0072 \mathrm{~g} / \mathrm{L}$. Calculate $K_{s p}$

Use the solubility rules (Table 4.1) to decide which of the following compounds are expected to be soluble and which insoluble. $a.\mathrm{NaBr}$ $\quad b.\mathrm{PbI}_2$ $\quad c.\mathrm{BaCO}_3$ $d.\left(\mathrm{NH}_4\right)_2 \mathrm{SO}_4$

You add dilute hydrochloric acid to a solution containing a metal ion. No precipitate forms. After the acidity is adjusted to $0.3 \mathrm{M}$ hydronium ion, you bubble hydrogen sulfide into the solution. Again no precipitate forms. Is it possible that the original solution contained silver ion? Could it have contained copper(II) ion?

You are given a solution of the ions $\mathrm{Mg}^{2+}, \mathrm{Ca}^{2+}$, and $\mathrm{Ba}^{2+}$. Devise a scheme to separate these ions using sodium sulfate. Note that magnesium sulfate is soluble.

When ammonia is first added to a solution of copper(II) nitrate, a pale blue precipitate of copper(II) hydroxide forms. As more ammonia is added, however, this precipitate dissolves. Describe what is happening.

Which of the following pictures best represents an unsaturated solution of sodium chloride, $\mathrm{NaCl}$ ? In these pictures, the dark gray spheres represent $\mathrm{Na}^{+}$ions and the green spheres represent chloride ions. For clarity, water molecules are not shown.