Multiple Choice
For which of the following mixtures will Ag2SO4(s) precipitate?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following compounds is insoluble in water according to common solubility rules?
A
K_2SO_4
B
NH_4Br
C
AgCl
D
NaNO_3
Verified step by step guidance1
Recall the common solubility rules for ionic compounds in water: most compounds containing alkali metal ions (like K\textsuperscript{+}) and the ammonium ion (NH\textsubscript{4}\textsuperscript{+}) are soluble.
Identify the ions in each compound: K\textsubscript{2}SO\textsubscript{4} contains K\textsuperscript{+} and SO\textsubscript{4}\textsuperscript{2-}, NH\textsubscript{4}Br contains NH\textsubscript{4}\textsuperscript{+} and Br\textsuperscript{-}, NaNO\textsubscript{3} contains Na\textsuperscript{+} and NO\textsubscript{3}\textsuperscript{-}, and AgCl contains Ag\textsuperscript{+} and Cl\textsuperscript{-}.
Apply the solubility rules: compounds with K\textsuperscript{+}, NH\textsubscript{4}\textsuperscript{+}, and NO\textsubscript{3}\textsuperscript{-} ions are generally soluble, so K\textsubscript{2}SO\textsubscript{4}, NH\textsubscript{4}Br, and NaNO\textsubscript{3} are soluble in water.
Recognize that silver chloride (AgCl) is a classic example of an insoluble salt in water, as most silver salts are insoluble except for a few exceptions.
Conclude that among the given compounds, AgCl is insoluble in water according to the common solubility rules.
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