Chapter 11

Determine the \(K_{\text {sp }}\) for the following sparingly soluble compounds, given their molar solubilities: (a) AgI, \(9.1 \times 10^{-9} \mathrm{~mol} \cdot \mathrm{L}^{-1}\); (b) \(\mathrm{Ca}(\mathrm{OH})_{2}\), \(0.011 \mathrm{~mol}-\mathrm{L}^{-1}\); (c) \(\mathrm{Ag}_{3} \mathrm{PO}_{4}, 2.7 \times 10^{-6} \mathrm{~mol}^{-\mathrm{L}}^{-1}\) (d) \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}, 5.2 \times 10^{-7} \mathrm{~mol} \cdot \mathrm{L}^{-1}\).

Limestone is composed primarily of calcium carbonate, A \(1.0-\mathrm{mm}^{3}\) chip of limestone was accidentally dropped into a water-filled swimming pool, measuring \(10 \mathrm{~m} \times 7 \mathrm{~m} \times 2 \mathrm{~m}\). Assuming that the carbonate ion does not function as a Bronsted base and that the \(\mathrm{pH}\) of the water is 7 , will the pebble dissolve entirely? The density of calcium carbonate is \(2.71 \mathrm{~g} \cdot \mathrm{cm}^{-3}\).

student finds on the shelf a bottle of a pure silver halide that could be AgCl or Agl. Devclop a simple chemical test that would allow the student to distinguish which compound was in the bottle.

A 20-mL sample of \(0.020 \mathrm{M} \mathrm{HCl}(\mathrm{aq})\) was titrated with \(0.035 \mathrm{M} \mathrm{KOH}(\mathrm{aq})\). Calculate the \(\mathrm{pH}\) at the following points in the titration and sketch the \(\mathrm{pH}\) curve: (a) no \(\mathrm{KOH}\) added; (b) \(5.00 \mathrm{~mL}\) of \(\mathrm{KOH}\) (aq) added; (c) an additional \(5.00 \mathrm{~mL}\) of \(\mathrm{KOH}\) (aq) (for a total of \(10.0 \mathrm{~mL}\).) added; (d) another \(5.0 \mathrm{~mL}\) of \(\mathrm{KOH}(\mathrm{aq})\) added; (e) another \(5.00 \mathrm{~mL}\). \(\mathrm{KOH}(\mathrm{aq})\) added. (f) Determine the volume of \(\mathrm{KOH}\) (aq) required to reach the stoichiometric point.

An old bottle labcled "Standardized \(6.0 \mathrm{M}\) \(\mathrm{NaOH}^{\prime \prime}\) was found on the back of a shelf in the stockroom. Over time, some of the NaOH had reacted with the glass and the solution was no longer \(6.0 \mathrm{M}\). To determine its purity, \(5.0 \mathrm{~mL}\) of the solution was diluted to \(100 \mathrm{ml}\). and titrated to the stoichiometric point with 11.8 mL. of \(2.05 \mathrm{M} \mathrm{HCl}(\mathrm{aq})\). What is the molarity of the sodium hydroxide solution?

The narcotic cocaine is a weak base wirh \(\mathrm{p} K_{\mathrm{b}}=5.59\). Calculate the ratio of the concentration of cocaine and its conjugate acid in a solution of \(\mathrm{pH}=8.00\).

Novocaine, which is used by dentists as a local anesthetic, is a weak base with \(\mathrm{pK}_{\mathrm{b}}=5.05\). Blood has a pH of \(7.4\). What is the ratio of concentrations of Novocaine to its conjugate acid in the bloodstream?

Will \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) precipitate from a solution formed from a mixture of \(100 \mathrm{~mL}\) of \(1.0 \times 10^{-4} \mathrm{M}\) \(\mathrm{AgNO}_{3}(\) aq \()\) and \(100 \mathrm{~mL}\) of \(1.0 \times 10^{-4} \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})\) ?

(a) Estimate the \(\mathrm{pH}\) of the solution that results when we add \(25.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{NaOH}(\mathrm{aq})\) to \(25.0 \mathrm{~mL}\) of \(0.125 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{3}\) (aq). (b) If we add an additional \(20.0 \mathrm{~mL}\) of the \(\mathrm{NaOH}(\mathrm{aq})\) solution, what would you predict the pH of the resulting solution to be?