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Chapter 24: Problem 76

The most soluble of the following solids in \(\mathrm{NH}_{3}(\mathrm{aq})\) is (a) \(\mathrm{Ca}(\mathrm{OH})_{2} ;\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2} ;\) (c) \(\mathrm{BaSO}_{4} ;\) (d) \(\mathrm{MgCO}_{3}\) (e) \(\overline{\mathrm{Fe}_{2} \mathrm{O}_{3}}\).

Short Answer

Expert verified
\(\mathrm{Cu}(\mathrm{OH})_{2}\)

Step by step solution

01

Understanding Solubility

Solubility is the ability of a solute to dissolve in a solvent. Ammonia has the ability to form complex ions with certain metal ions, hence increasing the solubility of their salts. In this case, it essentially transforms an otherwise insoluble salt into a soluble complex.
02

Checking Each Option

We need to check each given compound in the options to see which forms a complex ion with ammonia and hence, will be most soluble in \(\mathrm{NH}_{3}(\mathrm{aq})\). (a) \(\mathrm{Ca}(\mathrm{OH})_{2}\), (c) \(\mathrm{BaSO}_{4}\), (d) \(\mathrm{MgCO}_{3}\) and (e) \(\overline{\mathrm{Fe}_{2} \mathrm{O}_{3}}\) do not form stable complexes with ammonia. However, (b) \(\mathrm{Cu}(\mathrm{OH})_{2}\) forms a deep blue complex ion with ammonia, \(\mathrm{[Cu(NH}_{3}\mathrm{)_4]^{2+}}\) and is therefore, more soluble in ammonia than the other compounds.
03

Determining the Most Soluble Solid

The most soluble solid in \(\mathrm{NH}_{3}(\mathrm{aq})\), among the given options, is therefore, \(\mathrm{Cu}(\mathrm{OH})_{2}\).

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Most popular questions from this chapter

Of the following, the one that is a Bronsted-Lowry acid is (a) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} ;\) (b) \(\left[\mathrm{FeCl}_{4}\right]^{-} ;\) (c) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (d) \(\left[\mathrm{Zn}(\mathrm{OH})_{4}\right]^{-}\).

Describe how the crystal field theory explains the fact that so many transition metal compounds are colored.

Write the formula and name of (a) a complex ion having \(\mathrm{Cr}^{3+}\) as the central ion and two \(\mathrm{NH}_{3}\) molecules and four \(\mathrm{Cl}^{-}\) ions as ligands (b) a complex ion of iron(III) having a coordination number of 6 and \(\mathrm{CN}^{-}\) as ligands (c) a coordination compound comprising two types of complex ions: one a complex of \(\mathrm{Cr}(\mathrm{III})\) with ethylenediamine (en), having a coordination number of 6 the other, a complex of \(\mathrm{Ni}(\mathrm{II})\) with \(\mathrm{CN}^{-}\), having a coordination number of 4

Of the following complex ions, the one that is optically active is (a) \(\operatorname{cis}-\left[\operatorname{CoCl}_{2}(\text { en })_{2}\right]^{+} ;\) (b) \(\left[\operatorname{CoCl}_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{+}\) (c) \(\left[\mathrm{CoCl}_{4}\left(\mathrm{NH}_{3}\right)_{2}\right]^{-} ;(\mathrm{d})\left[\mathrm{CuCl}_{4}\right]^{-}\).

In your own words, describe the following terms or symbols: (a) coordination number; (b) \(\Delta_{\mathrm{o}} ;\) (c) ammine complex; (d) enantiomer.
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