If NaOH is added to an aqueous solution of zinc ions, a...

If $\mathrm{NaOH}$ is added to an aqueous solution of zinc ions, a white precipitate appears and on adding excess of $\mathrm{NaOH}$, the precipitate dissolves. In this solution, zinc exists in the (a) anionic part (b) cationic part (c) both in cationic and anionic parts (d) there is no zinc in the solution

If $\mathrm{NaOH}$ is added to an aqueous solution of zinc ions, a white precipitate appears and on adding excess of $\mathrm{NaOH}$, the precipitate dissolves. In this solution, zinc exists in the
(a) anionic part
(b) cationic part
(c) both in cationic and anionic parts
(d) there is no zinc in the solution

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Key Concepts

Precipitation and Dissolution Equilibria

Precipitation occurs when two ions in solution form an insoluble compound, as seen with zinc ions and hydroxide ions forming zinc hydroxide. However, when an excess of a reagent is added, the initially formed precipitate may undergo a secondary reaction that leads to its dissolution, indicating a dynamic equilibrium between solid and dissolved species.

Amphoteric Compounds

Amphoteric compounds can behave both as acids and bases. In inorganic chemistry, certain metal hydroxides, like zinc hydroxide, exhibit amphoteric behavior, meaning they can react with both acids and bases, which explains their ability to form precipitates and then dissolve in excess base.

Complex Ion Formation

Complex ion formation involves the coordination of additional ligands around a central metal ion, altering its solubility. In excess hydroxide, zinc hydroxide dissolves by forming the tetrahydroxozincate ion, an anionic complex, demonstrating how ligands affect the charge and solubility properties of metal species in solution.

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