Multiple Choice
Which of the following ions always form soluble ionic compounds in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following ions will form a precipitate when mixed with Pb^{2+} (lead(II) cation) in aqueous solution?
A
Cl^- (chloride ion)
B
SO_4^{2-} (sulfate ion)
C
NO_3^- (nitrate ion)
D
I^- (iodide ion)
Verified step by step guidance1
Recall that a precipitate forms when two ions combine to form an insoluble compound in water. To determine if a precipitate forms, we need to consider the solubility rules for common ionic compounds.
Identify the possible compounds formed when Pb^{2+} combines with each anion: PbCl_2, PbSO_4, Pb(NO_3)_2, and PbI_2.
Apply solubility rules: Nitrates (NO_3^-) are generally soluble, so Pb(NO_3)_2 will remain dissolved and not form a precipitate.
Chlorides (Cl^-) are mostly soluble, but PbCl_2 is only slightly soluble and may precipitate under certain conditions; sulfates (SO_4^{2-}) are mostly soluble, but PbSO_4 is sparingly soluble and can form a precipitate.
Iodides (I^-) with Pb^{2+} form PbI_2, which is known to be poorly soluble and will form a visible precipitate in aqueous solution.
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