91Ó°ÊÓ

A sample of \(0.96 \mathrm{~L}\) of \(\mathrm{HCl}\) at \(372 \mathrm{mmHg}\) and \(22^{\circ} \mathrm{C}\) is bubbled into \(0.034 \mathrm{~L}\) of \(0.57 M \mathrm{NH}_{3}\). What is the \(\mathrm{pH}\) of the resulting solution? Assume the volume of solution remains constant and that the \(\mathrm{HCl}\) is totally dissolved in the solution.

(a) Assuming complete dissociation and no ionpair formation, calculate the freezing point of a \(0.50 \mathrm{~m}\) NaI solution. (b) What is the freezing point after the addition of sufficient \(\mathrm{HgI}_{2},\) an insoluble compound, to the solution to react with all the free \(\mathrm{I}^{-}\) ions in solution? Assume volume to remain constant.

A \(1.0-\mathrm{L}\) saturated silver carbonate solution at \(5^{\circ} \mathrm{C}\) is treated with enough hydrochloric acid to decompose the compound. The carbon dioxide generated is collected in a \(19-\mathrm{mL}\) vial and exerts a pressure of \(114 \mathrm{mmHg}\) at \(25^{\circ} \mathrm{C}\). What is the \(K_{\mathrm{sp}}\) of \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) at \(5^{\circ} \mathrm{C} ?\)

A \(100-\mathrm{mL} 0.100 \mathrm{M} \mathrm{CuSO}_{4}\) solution is mixed with a \(100-\mathrm{mL} 0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution. Calculate the concentrations of the ions in the combined solution.

Use appropriate equations to account for the solubility of the amphoteric aluminum hydroxide \(\left.\left[\mathrm{Al}(\mathrm{OH})_{3}\right)\right]\) at low and high \(\mathrm{pHs}\)

From Table 16.2 we see that silver bromide (AgBr) has a larger solubility product than iron(II) hydroxide \(\left[\mathrm{Fe}(\mathrm{OH})_{2}\right] .\) Does this mean that \(\mathrm{AgBr}\) is more soluble than \(\mathrm{Fe}(\mathrm{OH})_{2} ?\)