Multiple Choice
Which of the following substances is most likely to dissolve in hexane?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which one of the following compounds will not be soluble in water?
A
NH4Br
B
AgCl
C
K2SO4
D
NaNO3
Verified step by step guidance1
Understand the general solubility rules for ionic compounds in water. Most compounds containing ammonium (NH4+), alkali metal ions (like K+ and Na+), and nitrates (NO3-) are soluble in water.
Check each compound against these rules: NH4Br contains NH4+ and Br-, both typically soluble; K2SO4 contains K+ and SO4^2-, and sulfates are generally soluble except with certain exceptions; NaNO3 contains Na+ and NO3-, both ions that form soluble compounds.
Identify common exceptions to sulfate solubility, such as sulfates of silver (Ag+), lead (Pb2+), and barium (Ba2+), which are poorly soluble.
Recognize that AgCl contains Ag+ and Cl-, and chlorides are generally soluble except for those of silver, lead, and mercury(I), making AgCl insoluble in water.
Conclude that among the given compounds, AgCl is the one that will not be soluble in water based on these solubility rules.
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