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Chapter 4: Problem 18

Specify what ions are present upon dissolving each of the following substances in water: (a) \(\mathrm{HIO}_{3},\) (b) \(\mathrm{Ba}(\mathrm{OH})_{2},\) (c) HCN, (d) \(\mathrm{CuSO}_{4}\).

Short Answer

Expert verified
Upon dissolving the given compounds in water, the following ions are formed: (a) \(\mathrm{HIO}_3\): \(\mathrm{H}^+\) and \(\mathrm{IO}_3^-\) (b) \(\mathrm{Ba(OH)_2}\): \(\mathrm{Ba}^{2+}\) and \(\mathrm{OH}^-\) (c) HCN: \(\mathrm{H}^+\) and \(\mathrm{CN}^-\) (in equilibrium) (d) \(\mathrm{CuSO}_4\): \(\mathrm{Cu}^{2+}\) and \(\mathrm{SO}_4^{2-}\)

Step by step solution

01

(a) Dissolving \(\mathrm{HIO}_3\)

When \(\mathrm{HIO}_3\) (iodic acid) is dissolved in water, it dissociates into its individual ions: a hydrogen ion (\(\mathrm{H}^+\)) and an iodate ion (\(\mathrm{IO}_3^-\)). The equation for this process is: \[\mathrm{HIO}_3(aq) \rightarrow \mathrm{H}^+(aq) + \mathrm{IO}_3^-(aq)\]
02

(b) Dissolving \(\mathrm{Ba(OH)_2}\)

Barium hydroxide, \(\mathrm{Ba(OH)_2}\), is a strong base and dissociates completely in water. It forms a barium ion (\(\mathrm{Ba}^{2+}\)) and two hydroxide ions (\(\mathrm{OH}^-\)). The equation for this process is: \[\mathrm{Ba(OH)_2}(aq) \rightarrow \mathrm{Ba}^{2+}(aq) + 2 \mathrm{OH}^-(aq)\]
03

(c) Dissolving HCN

Hydrogen cyanide (HCN) is a weak acid, meaning it does not dissociate completely in water. However, when it does dissociate, it forms a hydrogen ion (\(\mathrm{H}^+\)) and a cyanide ion (\(\mathrm{CN}^-\)). The equilibrium reaction is represented as: \[\mathrm{HCN}(aq) \rightleftharpoons \mathrm{H}^+(aq) + \mathrm{CN}^-(aq)\]
04

(d) Dissolving \(\mathrm{CuSO}_4\)

Copper(II) sulfate (\(\mathrm{CuSO}_4\)) is an ionic compound that dissociates completely in water. It forms a copper ion (\(\mathrm{Cu}^{2+}\)) and a sulfate ion (\(\mathrm{SO}_4^{2-}\)). The equation for this process is: \[\mathrm{CuSO}_4(aq) \rightarrow \mathrm{Cu}^{2+}(aq) + \mathrm{SO}_4^{2-}(aq)\] In summary, upon dissolving these compounds in water, the following ions are formed: (a) \(\mathrm{H}^+\), \(\mathrm{IO}_3^-\) (b) \(\mathrm{Ba}^{2+}\), \(\mathrm{OH}^-\) (c) \(\mathrm{H}^+\), \(\mathrm{CN}^-\) (in equilibrium) (d) \(\mathrm{Cu}^{2+}\), \(\mathrm{SO}_4^{2-}\)

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Most popular questions from this chapter

Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) HF, (b) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\) (benzoicacid), (c) \(\mathrm{C}_{6} \mathrm{H}_{6}\) (benzene), (d) \(\mathrm{CoCl}_{3}\) (e) \(\mathrm{AgNO}_{3}\)

The metal cadmium tends to form Cd \(^{2+}\) ions. The following observations are made: (i) When a strip of zinc metal is placed in $\mathrm{CdCl}_{2}(a q),$ cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q),\) nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations. (b) Which elements more closely define the position of cadmium in the activity series? (c) What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?

A solution of \(105.0 \mathrm{~mL}\) of \(0.300 \mathrm{M} \mathrm{NaOH}\) is mixed with a solution of \(150.0 \mathrm{~mL}\) of \(0.060 \mathrm{MAlCl}_{3} .\) (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?

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(a) Is the number of moles of ions present in a solution an intensive or an extensive property? (b) Can you identify which one between $0.10 \mathrm{~mol} \mathrm{ZnCl}_{2}\( and \)0.1 \mathrm{M} \mathrm{ZnCl}_{2}$ contains more \(\mathrm{Zn}^{2+}\) ion? Why?
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