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Chapter 18: Problem 97

All but two of the following solutions yield a precipitate when the solution is also made \(2.00 \mathrm{M}\) in \(\mathrm{NH}_{3}\). Those two are (a) \(\mathrm{MgCl}_{2}(\mathrm{aq}) ;\) (b) \(\mathrm{FeCl}_{3}(\mathrm{aq})\); (c) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(\mathrm{aq}) ;(\mathrm{d}) \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})\); (e) \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(\mathrm{aq})\).

Short Answer

Expert verified
The two solutions that will not form a precipitate when the solution is made 2.00M in \(NH_3\) are: (c) \((NH_4)_2SO_4\) and (d) \(Cu(NO_3)_2\).

Step by step solution

01

Identify the possible precipitates

Using knowledge of solubility rules, the possible salts that can form a precipitate were identified. These are: 1. \(MgCl_2\)2. \(FeCl_3\)3. \(Cu(NO_3)_2\)4. \(Al_2(SO_4)_3\)
02

Identify the soluble salts in ammonia

The rules of solubility show that most nitrate (NO3) salts and most ammonium (NH4) salts are soluble. Therefore, \(NH_4)_2SO_4\) and \(Cu(NO_3)_2\) will not form a precipitate when the solution is made 2.00M in \(NH_3\)

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Most popular questions from this chapter

Calculate the molar solubility of \(\mathrm{Mg}(\mathrm{OH})_{2}\) \(\left(K_{\mathrm{sp}}=1.8 \times 10^{-11}\right)\) in (a) pure water; (b) \(0.0862 \mathrm{M}\) \(\mathrm{MgCl}_{2} ;\) (c) \(0.0355 \mathrm{M} \mathrm{KOH}(\mathrm{aq})\).

\(\mathrm{KI}(\mathrm{aq})\) is slowly added to a solution with \(\left[\mathrm{Pb}^{2+}\right]=\) \(\left[\mathrm{Ag}^{+}\right]=0.10 \mathrm{M} .\) For \(\mathrm{PbI}_{2}, K_{\mathrm{sp}}=7.1 \times 10^{-9} ;\) for \(\mathrm{AgI},\) \(K_{\mathrm{sp}}=8.5 \times 10^{-17}\). (a) Which precipitate should form first, \(\mathrm{PbI}_{2}\) or AgI? (b) What \(\left[\mathrm{I}^{-}\right]\) is required for the second cation to begin to precipitate? (c) What concentration of the first cation to precipitate remains in solution at the point at which the second cation begins to precipitate? (d) \(\operatorname{Can} \mathrm{Pb}^{2+}(\mathrm{aq})\) and \(\mathrm{Ag}^{+}(\) aq) be effectively separated by fractional precipitation of their iodides?

The slightly soluble solute \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\) is most soluble in (a) pure water; (b) \(0.10 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4} ;\) (c) \(0.25 \mathrm{M} \mathrm{KNO}_{3}\); (d) \(0.40 \mathrm{M} \mathrm{AgNO}_{3}\).

A solution is \(0.05 \mathrm{M}\) in \(\mathrm{Cu}^{2+},\) in \(\mathrm{Hg}^{2+},\) and in \(\mathrm{Mn}^{2+}\). Which sulfides will precipitate if the solution is made to be \(0.10 \mathrm{M} \mathrm{H}_{2} \mathrm{S}(\mathrm{aq})\) and \(0.010 \mathrm{M} \mathrm{HCl}(\mathrm{aq}) ?\) For \(\mathrm{CuS}\), \(K_{\mathrm{spa}}=6 \times 10^{-16} ;\) for \(\mathrm{HgS}, K_{\mathrm{spa}}=2 \times 10^{-32} ;\) for \(\mathrm{MnS}\), \(K_{\mathrm{spa}}=3 \times 10^{7}\).

Will precipitation of \(\mathrm{MgF}_{2}(\mathrm{s})\) occur if a \(22.5 \mathrm{mg}\) sample of \(\mathrm{MgCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) is added to \(325 \mathrm{mL}\) of \(0.035 \mathrm{M} \mathrm{KF}\) ?
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