Multiple Choice
Which of the following compounds is more soluble in an acidic solution than in a neutral solution?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
Multiple Choice
Which of the following ionic compounds is soluble in water?
A
BaSO_4
B
PbSO_4
C
AgCl
D
NaNO_3
Verified step by step guidance1
Understand the concept of solubility: Solubility in water depends on the ability of the ionic compound to dissociate into its ions and interact favorably with water molecules. Generally, compounds containing alkali metal ions (like Na\+) and nitrate ions (NO_3\-) are highly soluble in water.
Recall common solubility rules: For sulfates (SO_4^{2-}), most are soluble except those with Ba^{2+}, Pb^{2+}, and a few others, which are generally insoluble or sparingly soluble. For chlorides (Cl^-), most are soluble except those with Ag^+, Pb^{2+}, and Hg_2^{2+}.
Analyze each compound given: BaSO_4 and PbSO_4 are sulfates with Ba^{2+} and Pb^{2+}, which are exceptions to sulfate solubility and thus are not very soluble. AgCl contains Ag^+, which forms an insoluble chloride.
Compare with NaNO_3: Sodium nitrate contains Na^+ (an alkali metal ion) and NO_3^- (nitrate ion), both of which form compounds that are generally soluble in water without exceptions.
Conclude that among the options, NaNO_3 is soluble in water because it follows the solubility rules for alkali metal nitrates, while BaSO_4, PbSO_4, and AgCl are not soluble due to their respective ions causing low solubility.
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