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Chapter 5: Problem 19

Complete each of the following as a net ionic equation, indicating whether a precipitate forms. If no reaction occurs, so state. (a) $\mathrm{Na}^{+}+\mathrm{Br}^{-}+\mathrm{Pb}^{2+}+2 \mathrm{NO}_{3}^{-} \longrightarrow$ (b) $\mathrm{Mg}^{2+}+2 \mathrm{Cl}^{-}+\mathrm{Cu}^{2+}+\mathrm{SO}_{4}^{2-} \longrightarrow$ (c) $\mathrm{Fe}^{3+}+3 \mathrm{NO}_{3}^{-}+\mathrm{Na}^{+}+\mathrm{OH}^{-} \longrightarrow$

Short Answer

Expert verified
The net ionic equation for options (a), (b), and (c) are: (a) \( Pb^{2+} + 2 Br^{-} \longrightarrow PbBr2_{(s)} \), (b) No Reaction Occurs, and (c) No Reaction Occurs respectively.

Step by step solution

01

Determine if Formed Compounds are Soluble for (a)

For the reaction \(Na^{+} + Br^{-} + Pb^{2+} + 2 NO_{3}^{-}\), we have to check if the resultant lead bromide (PbBr2) and sodium nitrate (NaNO3) are soluble in water. From solubility rules, we know that most nitrates are soluble and most lead (II) compounds, except Pb(NO3)2 and Pb(C2H3O2)2, are insoluble.
02

Formulate Net Ionic Equation for (a)

Given that PbBr2 is insoluble and NaNO3 is soluble, the net ionic equation will be written as follows: \(Pb^{2+} + 2 Br^{-} \longrightarrow PbBr2_{(s)}\) indicating the formation of a precipitate.
03

Determine if Formed Compounds are Soluble for (b)

For the reaction \( Mg^{2+} + 2 Cl^{-} + Cu^{2+} + SO_{4}^{2-} \), we need to check if the resultant magnesium chlorate (MgCl2) and copper sulfate (CuSO4) are soluble. From solubility rules, we know that most sulfate salts are soluble, except for those with Ba^2+, Pb^2+, Hg2^2+, and Sr^2+. Chlorides are generally soluble, exceptions includes Ag+, Pb2+, and Hg2^2+.
04

Formulate Net Ionic Equation for (b)

Given that both MgCl2 and CuSO4 are soluble, no reaction occurs in this scenario, so we state that no reaction occurs.
05

Determine if Formed Compounds are Soluble for (c)

For the reaction \( Fe^{3+} + 3 NO_{3}^{-} + Na^{+} + OH^{-} \), we have to check if the resultant iron (III) nitrate (Fe(NO3)3) and sodium hydroxide (NaOH) are soluble. From solubility rules, we know that most hydroxides are insoluble, but group 1 element hydroxides (like NaOH) and Ba(OH)2 are soluble. Also, nitrates are generally soluble.
06

Formulate Net Ionic Equation for (c)

Given that NaOH and Fe(NO3)3 are soluble, no reaction occurs in this scenario, so we state that no reaction occurs.

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Most popular questions from this chapter

The titration of \(5.00 \mathrm{mL}\) of a saturated solution of sodium oxalate, \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) at \(25^{\circ} \mathrm{C}\) requires \(25.8 \mathrm{mL}\) of \(0.02140 \mathrm{M} \mathrm{KMnO}_{4}\) in acidic solution. What mass of \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) in grams would be present in \(1.00 \mathrm{L}\) of this saturated solution? \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}+\mathrm{MnO}_{4}^{-} \longrightarrow_{\mathrm{Mn}^{2+}}+\mathrm{CO}_{2}(\mathrm{g}) \quad\) (not balanced)

Select the (a) best and (b) poorest electrical conductors from the following solutions, and explain the reason for your choices: \(0.10 \mathrm{M} \mathrm{NH}_{3} ; 0.10 \mathrm{M} \mathrm{NaCl} ; 0.10 \mathrm{M}\) \(\mathrm{CH}_{3} \mathrm{COOH}\) (acetic acid); \(0.10 \mathrm{M} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (ethanol).

Assuming the volumes are additive, what is the \(\left[\mathrm{Cl}^{-}\right]\) in a solution obtained by mixing \(225 \mathrm{mL}\) of \(0.625 \mathrm{M}\) \(\mathrm{KCl}\) and \(615 \mathrm{mL}\) of \(0.385 \mathrm{M} \mathrm{MgCl}_{2} ?\)

Which of the following reactions are oxidationreduction reactions? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})\) (b) \(2 \mathrm{Li}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(1) \longrightarrow 2 \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})\) (c) \(4 \mathrm{Ag}(\mathrm{s})+\mathrm{PtCl}_{4}(\mathrm{aq}) \longrightarrow 4 \mathrm{AgCl}(\mathrm{s})+\mathrm{Pt}(\mathrm{s})\) (d) \(2 \mathrm{HClO}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \longrightarrow\) \(2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(\mathrm{aq})\)

Iron (Fe) is obtained from rock that is extracted from open pit mines and then crushed. The process used to obtain the pure metal from the crushed rock produces solid waste, called tailings, which are stored in disposal areas near the mines. The tailings pose a serious environmental risk because they contain sulfides, such as pyrite ( \(\mathrm{FeS}_{2}\) ), which oxidize in air to produce metal ions and \(\mathrm{H}^{+}\) ions that can enter into surface water or ground water. The oxidation of \(\mathrm{FeS}_{2}\) to \(\mathrm{Fe}^{3+}\) is described by the unbalanced chemical equation below. \(\mathrm{FeS}_{2}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow\) \(\quad \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \quad(\text { not balanced })\) Thus, the oxidation of pyrite produces \(\mathrm{Fe}^{3+}\) and \(\mathrm{H}^{+}\) ions that can leach into surface or ground water. The leaching of \(\mathrm{H}^{+}\) ions causes the water to become very acidic. To prevent acidification of nearby ground or surface water, limestone \(\left(\mathrm{CaCO}_{3}\right)\) is added to the tailings to neutralize the \(\mathrm{H}^{+}\) ions: \(\mathrm{CaCO}_{3}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \underset{\mathrm{Ca}^{2+}}{\longrightarrow}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g})\) (a) Balance the equation above for the reaction of \(\mathrm{FeS}_{2}\) and \(\mathrm{O}_{2}\). [ Hint: Start with the half-equations \(\mathrm{FeS}_{2}(\mathrm{s}) \rightarrow\) \(\left.\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq}) \text { and } \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(1) .\right]\) (b) What is the minimum amount of \(\mathrm{CaCO}_{3}(\mathrm{s})\) required, per kilogram of tailings, to prevent contamination if the tailings contain \(3 \%\) S by mass? Assume that all the sulfur in the tailings is in the form \(\mathrm{FeS}_{2}\).
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