Multiple Choice
For which of the following mixtures will Ag2SO4(s) precipitate?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
Multiple Choice
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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