Problem 63
Which insoluble compound in each pair should be more soluble in nitric acid than in pure water? (a) \(\mathrm{PbCl}_{2}\) or \(\mathrm{PbS}\) (b) \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) or \(\mathrm{AgI}\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}\) or \(\mathrm{AgCl}\)
Problem 64
Which compound in each pair is more soluble in water than is predicted by a calculation from \(K_{\mathrm{sp}} ?\) (a) AgI or \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{PbCO}_{3}\) or \(\mathrm{PbCl}_{2}\) (c) AgCl or AgCN
Problem 65
You have a solution that has a lead(II) ion concentration of 0.0012 M. If enough soluble chloride-containing salt is added so that the \(\mathrm{Cl}^{-}\) concentration is 0.010 \(\mathrm{M},\) will \(\mathrm{PbCl}_{2}\) precipitate?
Problem 68
You have \(95 \mathrm{mL}\) of a solution that has a lead(II) concentration of 0.0012 M. Will PbCl_ precipitate when 1.20 g of solid \(\mathrm{NaCl}\) is added?
Problem 70
Will a precipitate of \(\mathrm{Mg}(\mathrm{OH})_{2}\) form when \(25.0 \mathrm{mL}\) of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M solution of magnesium chloride?
Problem 77
In each of the following cases, decide whether a precipitate will form when mixing the indicated reagents, and write a balanced equation for the reaction. (a) \(\mathrm{NaBr}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq})\) (b) \(\mathrm{KCl}(\mathrm{aq})+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})\)
Problem 78
In each of the following cases, decide whether a precipitate will form when mixing the indicated reagents, and write a balanced equation for the reaction. (a) \(\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})\) (b) \(\mathrm{K}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{FeCl}_{3}(\mathrm{aq})\)
Problem 79
If you mix 48 mL of \(0.0012 \mathrm{M} \mathrm{BaCl}_{2}\) with \(24 \mathrm{mL}\) of \(1.0 \times 10^{-6} \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4},\) will a precipitate of \(\mathrm{BaSO}_{4}\) form?
Problem 80
Calculate the hydronium ion concentration and the pH of the solution that results when \(20.0 \mathrm{mL}\) of \(0.15 \mathrm{M}\) acetic acid, \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H},\) is mixed with \(5.0 \mathrm{mL}\) of \(0.17 \mathrm{M} \mathrm{NaOH}.\)
Problem 82
For each of the following cases, decide whether the pH is less than \(7,\) equal to \(7,\) or greater than 7. (a) Equal volumes of 0.10 M acetic acid, \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H},\) and \(0.10 \mathrm{M} \mathrm{KOH}\) are mixed. (b) \(25 \mathrm{mL}\) of \(0.015 \mathrm{M} \mathrm{NH}_{3}\) is mixed with \(12 \mathrm{mL}\) of 0.015 M HCl. (c) 150 mL of \(0.20 \mathrm{M} \mathrm{HNO}_{3}\) is mixed with \(75 \mathrm{mL}\) of 0.40 M NaOH. (d) \(25 \mathrm{mL}\) of \(0.45 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) is mixed with \(25 \mathrm{mL}\) of 0.90 M NaOH.
