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Chapter 21: Problem 5

Arrange the following compounds in the expected order of increasing solubility in water, and give the basis for your arrangement: \(\mathrm{Li}_{2} \mathrm{CO}_{3}, \mathrm{Na}_{2} \mathrm{CO}_{3}\) \(\mathrm{MgCO}_{3}.\)

Short Answer

Expert verified
The compounds in increasing order of solubility are: \(\mathrm{MgCO}_{3}<\mathrm{Li}_{2}\mathrm{CO}_{3}<\mathrm{Na}_{2}\mathrm{CO}_{3}\)

Step by step solution

01

Understand solubility rules

Solubility rules state that all alkali metal salts are soluble. Alkali metals include lithium (Li), sodium (Na), potassium (K), rubidium (Rb) and cesium (Cs). Carbonates are usually insoluble except those of alkali metals and ammonium ion (NH4+). Among alkali metals, lithium salts are less soluble than sodium salts. Thus, \(\mathrm{Li}_{2}\mathrm{CO}_{3}\) should be less soluble than \(\mathrm{Na}_{2}\mathrm{CO}_{3}\). Magnesium carbonate (\(\mathrm{MgCO}_{3}\)) is largely insoluble in water.
02

Arrange the compounds

Based on the solubility rules, the given compounds should be arranged in increasing order of their solubility in water as follows: \(\mathrm{MgCO}_{3}<\mathrm{Li}_{2}\mathrm{CO}_{3}<\mathrm{Na}_{2}\mathrm{CO}_{3}\)

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Most popular questions from this chapter

Briefly describe each of the following ideas, methods, or phenomena: (a) diagonal relationship; (b) preparation of deionized water by ion exchange; (c) thermite reaction; (d) inert pair effect.

Lithium superoxide, \(\mathrm{LiO}_{2}(\mathrm{s}),\) has never been isolated. Use ideas from Chapter \(12,\) together with data from this chapter and Appendix \(D\), to estimate \(\Delta H_{f}\) for \(\mathrm{LiO}_{2}(\mathrm{s})\) and assess whether \(\mathrm{LiO}_{2}(\mathrm{s})\) is thermodynamically stable with respect to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}).\) (a) Use the Kapustinskii equation, along with appropriate data below, to estimate the lattice energy, \(U,\) for \(\left.\mathrm{LiO}_{2}(\mathrm{s}) . \text { (See exercise } 126 \text { in Chapter } 12 .\right)\) The ionic radii for \(L\) i \(^{+}\) and \(O_{2}^{-}\) are \(73 \mathrm{pm}\) and \(144 \mathrm{pm},\) respectively. (b) Use your result from part (a) in the BornFajans-Haber cycle to estimate \(\Delta H_{\mathrm{f}}^{2}\) for \(\mathrm{LiO}_{2}(\mathrm{s})\) [Hint: For the process \(\mathrm{O}_{2}(\mathrm{g})+\mathrm{e}^{-} \rightarrow \mathrm{O}_{2}^{-}(\mathrm{g}), \Delta H^{\circ}=.\) \(-43 \mathrm{kJ} \mathrm{mol}^{-1} .\) See Table 21.2 and Appendix \(\mathrm{D}\) for the other data that are required.] (c) Use your result from part (b) to calculate the enthalpy change for the decomposition of \(\mathrm{LiO}_{2}(\mathrm{s})\) to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}) .\) For \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s}), \Delta H_{\mathrm{f}}^{\circ}=-598.73\) \(\mathrm{kJmol}^{-1}.\) (d) Use your result from part (c) to decide whether \(\mathrm{LiO}_{2}(\mathrm{s})\) is thermodynamically stable with respect to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}) .\) Assume that entropy effects can be neglected.

Of the following oxides, the one with the highest melting point is (a) \(\mathrm{Li}_{2} \mathrm{O} ;\) (b) \(\mathrm{BaO} ;\) (c) \(\mathrm{MgO} ;\) (d) \(\mathrm{SiO}_{2}.\)

The Gibbs energies of formation, \(\Delta G_{f}^{Q}\), for \(\mathrm{KO}_{2}(\mathrm{s})\) and \(\mathrm{K}_{2} \mathrm{O}(\mathrm{s})\) are \(-240.59 \mathrm{kJmol}^{-1}\) and \(-322.09 \mathrm{kJmol}^{-1}\) respectively, at \(298 \mathrm{K}\). Calculate the equilibrium constant for the reaction below at \(298 \mathrm{K}\). Is \(\mathrm{KO}_{2}(\mathrm{s})\) thermodynamically stable with respect to \(\mathrm{K}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g})\) at \(298 \mathrm{K} ?\) $$ 2 \mathrm{KO}_{2}(\mathrm{s}) \longrightarrow \mathrm{K}_{2} \mathrm{O}(\mathrm{s})+\frac{3}{2} \mathrm{O}_{2}(\mathrm{g}) $$

Write plausible chemical equations for the (a) dissolving of lead(II) oxide in nitric acid; (b) heating of \(\operatorname{snCO}_{3}(\mathrm{s}) ;\) (c) reduction of lead(II) oxide by carbon; (d) reduction of \(\mathrm{Fe}^{3+}(\mathrm{aq})\) to \(\mathrm{Fe}^{2+}(\mathrm{aq})\) by \(\mathrm{Sn}^{2+}(\mathrm{aq});\) (e) formation of lead(II) sulfate during high-temperature roasting of lead(II) sulfide.
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