Question

question 9
1 pts
it is possible to predict the solubility of a given ionic compound based on patterns observed for a other ionic compounds.
based on these patterns (table 7.1 ), which of the following compounds would be expected to be soluble? (pick all that apply)
compounds containing lead(ii) ions
compounds containing nitrate ions
compounds containing silver ions
compounds containing group i cations
compounds containing acetate ions

Explanation:

• Compounds containing nitrate ions (\(NO_3^-\)) are generally soluble.
• Compounds containing group I cations (e.g., \(Li^+\), \(Na^+\), \(K^+\) etc.) are soluble.
• Compounds containing acetate ions (\(CH_3COO^-\)) are soluble.
• Compounds containing lead(II) ions (\(Pb^{2+}\)) are mostly insoluble (e.g., \(PbCl_2\), \(PbSO_4\) etc., though some \(Pb^{2+}\) compounds like \(Pb(NO_3)_2\) are soluble but it's an exception and not a general rule for \(Pb^{2+}\) compounds).
• Compounds containing silver ions (\(Ag^+\)) are mostly insoluble (e.g., \(AgCl\), \(AgBr\), \(AgI\), \(Ag_2CO_3\) etc., though \(AgNO_3\) is soluble but it's an exception for \(Ag^+\) compounds).

Answer:

• Compounds containing nitrate ions
• Compounds containing group I cations
• Compounds containing acetate ions