Question

which of the following ion/ions are soluble except ag+? c₂h₃o₂⁻ cl⁻, br⁻, i⁻ oh⁻ so₄⁻²

Explanation:

Step1: Analyze acetate ion (\(C_{2}H_{3}O_{2}^{-}\)) solubility

According to solubility rules, most acetates are soluble. Silver acetate (\(AgC_{2}H_{3}O_{2}\)) has a relatively low solubility compared to acetates of alkali metals, but it is still more soluble than many silver - halide, silver - hydroxide and silver - sulfate compounds.

Step2: Analyze halide ions (\(Cl^{-}, Br^{-}, I^{-}\)) solubility with \(Ag^{+}\)

Silver chloride (\(AgCl\)), silver bromide (\(AgBr\)) and silver iodide (\(AgI\)) are insoluble in water. The solubility product constants (\(K_{sp}\)) of these compounds are very small (\(K_{sp}(AgCl)=1.8\times10^{-10}\), \(K_{sp}(AgBr) = 5.0\times10^{-13}\), \(K_{sp}(AgI)=8.3\times10^{-17}\))

Step3: Analyze hydroxide ion (\(OH^{-}\)) solubility with \(Ag^{+}\)

Silver hydroxide (\(AgOH\)) is unstable and decomposes to form silver oxide (\(Ag_{2}O\)) in water. In a sense, we can consider \(AgOH\) as insoluble (the decomposition reaction \(2AgOH=Ag_{2}O + H_{2}O\) occurs because of the low stability of \(AgOH\))

Step4: Analyze sulfate ion (\(SO_{4}^{2 - }\)) solubility with \(Ag^{+}\)

Silver sulfate (\(Ag_{2}SO_{4}\)) has a \(K_{sp}=1.2\times 10^{-5}\). While it is more soluble than \(AgCl\), \(AgBr\), \(AgI\) and \(AgOH\) (or its decomposition product), it is still less soluble than most acetates

Answer:

\(C_{2}H_{3}O_{2}^{-}\)