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Chapter 22: Problem 66
Write an appropriate formula for each of the following: (a) hydroxylamine; (b) calcium hydrogen phosphate; (c) lithium nitride.
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Give a specific example of a chemical equation that illustrates the (a) reaction of a metal sulfide with \(\mathrm{HCl}(\mathrm{aq})\) (b) action of a nonoxidizing acid on a metal sulfite; (c) oxidation of \(\mathrm{SO}_{2}(\mathrm{aq})\) to \(\mathrm{SO}_{4}^{2-}(\mathrm{aq})\) by \(\mathrm{MnO}_{2}(\mathrm{s})\) in acidic solution; (d) disproportionation of \(S_{2} \mathrm{O}_{3}^{2-}\) in acidic solution.
Give an appropriate formula for each of the following compounds: (a) calcium sulfate dihydrate; (b) hydrosulfuric acid; (c) sodium hydrogen sulfate; (d) disulfuric acid.
The heavier halogens (Cl, Br, and I) form compounds in which the central halogen atom, \(X\), is bonded directly to oxygen and to fluorine. Several examples are known, including those with formulas of the type \(\mathrm{FXO}_{2}, \mathrm{FXO}_{3, \text { and } \mathrm{F}_{3} \mathrm{XO} . \text { The structures of these }}\) molecules are all consistent with the VSEPR model. Draw Lewis structures and predict the geometries of (a) chloryl fluoride, \(\mathrm{FClO}_{2}\); (b) perchloryl fluoride, \(\mathrm{FClO}_{3} ;(\mathrm{c}) \mathrm{F}_{3} \mathrm{ClO}\).
A 25.0 L sample of a natural gas, measured at \(25^{\circ} \mathrm{C}\). and 740.0 Torr, is bubbled through \(\mathrm{Pb}^{2+}(\mathrm{aq}),\) yielding \(0.535 \mathrm{g}\) of \(\mathrm{PbS}(\mathrm{s}) .\) What mass of sulfur can be recovered per cubic meter of this natural gas?
\(\mathrm{O}_{3}(\mathrm{g})\) is a powerful oxidizing agent. Write equations to represent oxidation of \((a) I^{-}\) to \(I_{2}\) in acidic solution; (b) sulfur in the presence of moisture to sulfuric acid; (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) to \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) in basic solution. In each case \(\mathrm{O}_{3}(\mathrm{g})\) is reduced to \(\mathrm{O}_{2}(\mathrm{g})\).
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