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Chapter 18: Problem 6

Which of the following saturated aqueous solutions would have the highest \(\left[\mathrm{Mg}^{2+}\right]\): (a) \(\mathrm{MgCO}_{3} ;\) (b) \(\mathrm{MgF}_{2};\) (c) \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2} ?\) Explain.

Short Answer

Expert verified
The exact answer depends on the \(K_{sp}\) values for the three compounds, which may vary between different sources. The student must find these values from a reliable source to complete the exercise.

Step by step solution

01

Find the Ksp values

Search for the solubility product constants (\(K_{sp}\)) for the given compounds. \(K_{sp}\) values are typically listed in chemistry textbooks or online sources.
02

Compare the Ksp values

Compare the \(K_{sp}\) values of the three compounds. The compound with the highest \(K_{sp}\) will have the highest concentration of \( \mathrm{Mg}^{2+}\) ions in a saturated solution.
03

Identify the compound

The compound with the highest \(K_{sp}\) value is the one that will produce the highest [\(\mathrm{Mg}^{2+}]\) concentration in solution.

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Most popular questions from this chapter

In the Mohr titration, \(\mathrm{Cl}^{-}(\mathrm{aq})\) is titrated with \(\mathrm{AgNO}_{3}(\text { aq })\) in solutions that are at about \(\mathrm{pH}=7\). Thus, it is suitable for determining the chloride ion content of drinking water. The indicator used in the titration is \(\mathrm{K}_{2} \mathrm{CrO}_{4}(\text { aq }) .\) A red-brown precipitate of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})\) forms after all the \(\mathrm{Cl}^{-}\) has precipitated. The titration reaction is \(\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \longrightarrow \mathrm{AgCl}(\mathrm{s}) .\) At the equivalence point of the titration, the titration mixture consists of \(\mathrm{AgCl}(\mathrm{s})\) and a solution having neither \(\mathrm{Ag}^{+}\) nor \(\mathrm{Cl}^{-}\) in excess. Also, no \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})\) is present, but it forms immediately after the equivalence point. (a) How many milliliters of \(0.01000 \mathrm{M} \mathrm{AgNO}_{3}(\mathrm{aq})\) are required to titrate \(100.0 \mathrm{mL}\) of a municipal water sample having \(29.5 \mathrm{mg} \mathrm{Cl}^{-} / \mathrm{L} ?\) (b) What is \(\left[\mathrm{Ag}^{+}\right]\) at the equivalence point of the Mohr titration? (c) What is \(\left[\mathrm{CrO}_{4}^{2-}\right]\) in the titration mixture to meet the requirement of no precipitation of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})\) until immediately after the equivalence point? (d) Describe the effect on the results of the titration if \(\left[\mathrm{CrO}_{4}^{2-}\right]\) were (1) greater than that calculated in part (c) or (2) less than that calculated? (e) Do you think the Mohr titration would work if the reactants were exchanged - that is, with \(\mathrm{Cl}^{-}(\text {aq })\) as the titrant and \(\mathrm{Ag}^{+}(\) aq) in the sample being analyzed? Explain.

\(\mathrm{AgNO}_{3}(\mathrm{aq})\) is slowly added to a solution that is \(0.250 \mathrm{M}\) \(\mathrm{NaCl}\) and also \(0.0022 \mathrm{M} \mathrm{KBr}\). (a) Which anion will precipitate first, \(\mathrm{Cl}^{-}\) or \(\mathrm{Br}^{-}\) ? (b) What is \(\left[\mathrm{Ag}^{+}\right]\) at the point at which the second anion begins to precipitate? (c) Can the \(\mathrm{Cl}^{-1}\) and \(\mathrm{Br}^{-}\) be separated effectively by this fractional precipitation?

What is the minimum \(\mathrm{pH}\) at which \(\mathrm{Cr}(\mathrm{OH})_{3}(\mathrm{s})\) will precipitate from a solution that is \(0.086 \mathrm{M}\) in \(\mathrm{Cr}^{3+}(\mathrm{aq}) ?\)

A solution is \(0.10 \mathrm{M}\) in free \(\mathrm{NH}_{3}, 0.10 \mathrm{M}\) in \(\mathrm{NH}_{4} \mathrm{Cl}\), and \(0.015 \mathrm{M}\) in \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} .\) Will \(\mathrm{Cu}(\mathrm{OH})_{2}(\mathrm{s})\) precipitate from this solution? \(K_{\mathrm{sp}}\) of \(\mathrm{Cu}(\mathrm{OH})_{2}\) is \(2.2 \times 10^{-20}\).

A solution is saturated with magnesium palmitate \(\left[\mathrm{Mg}\left(\mathrm{C}_{16} \mathrm{H}_{31} \mathrm{O}_{2}\right)_{2}, \text { a component of bathtub ring }\right] \mathrm{at}\) \(50^{\circ} \mathrm{C} .\) How many milligrams of magnesium palmitate will precipitate from \(965 \mathrm{mL}\) of this solution when it is cooled to \(25^{\circ} \mathrm{C} ?\) For \(\mathrm{Mg}\left(\mathrm{C}_{16} \mathrm{H}_{31} \mathrm{O}_{2}\right)_{2},\) \(K_{\mathrm{sp}}=4.8 \times 10^{-12}\) at \(50^{\circ} \mathrm{C}\) and \(3.3 \times 10^{-12}\) at \(25^{\circ} \mathrm{C}\).
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