Write balanced net ionic equations for the following...

Write balanced net ionic equations for the following reactions in basic solution: (a) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}(a q)+\mathrm{I}_{2}(a q) \longrightarrow \mathrm{S}_{4} \mathrm{O}_{6}^{2-}(a q)+\mathrm{I}^{-}(a q)$ (b) $\mathrm{Mn}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{MnO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l)$ (c) $\mathrm{Zn}(s)+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NH}_{3}(a q)+\mathrm{Zn}(\mathrm{OH})_{4}^{2-}(a q)$ (d) $\mathrm{Bi}(\mathrm{OH})_{3}(s)+\mathrm{Sn}(\mathrm{OH})_{3}^{-}(a q) \longrightarrow \mathrm{Bi}(s)+\mathrm{Sn}(\mathrm{OH})_{6}^{2-}(a q)$

Write balanced net ionic equations for the following reactions in basic solution:
(a) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}(a q)+\mathrm{I}_{2}(a q) \longrightarrow \mathrm{S}_{4} \mathrm{O}_{6}^{2-}(a q)+\mathrm{I}^{-}(a q)$
(b) $\mathrm{Mn}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{MnO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l)$
(c) $\mathrm{Zn}(s)+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NH}_{3}(a q)+\mathrm{Zn}(\mathrm{OH})_{4}^{2-}(a q)$
(d) $\mathrm{Bi}(\mathrm{OH})_{3}(s)+\mathrm{Sn}(\mathrm{OH})_{3}^{-}(a q) \longrightarrow \mathrm{Bi}(s)+\mathrm{Sn}(\mathrm{OH})_{6}^{2-}(a q)$

Key Concepts

Net Ionic Equations

Net ionic equations show only the species that actually participate in a chemical change, eliminating spectator ions that do not undergo transformation during the reaction. This concept is central to understanding the true chemical process, as it highlights the essence of the reaction without the clutter of ions that simply balance the charge.

Redox Reactions

Redox reactions involve the transfer of electrons between chemical species leading to changes in their oxidation states. Recognizing and understanding redox processes is crucial because it allows one to determine which species are oxidized and which are reduced, forming the basis for writing balanced net ionic equations in redox chemistry.

Half-Reaction Method

The half-reaction method is a systematic approach used to balance complex redox equations by dividing the overall reaction into oxidation and reduction half reactions. Each half reaction is balanced separately for mass and charge, including electrons, and then recombined to yield the fully balanced net ionic equation.

Balancing Reactions in Basic Solution

Balancing reactions in basic solution requires additional steps compared to acidic conditions, primarily the addition of hydroxide ions (OH–) to neutralize hydrogen ions (H+) when they appear during the balancing process. This concept ensures that the final equation accurately reflects the conditions of the reaction medium, with water and hydroxide ions used appropriately to achieve a balanced equation under basic conditions.

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