Multiple Choice
Which of the following ions is most likely to form an insoluble sulfate compound?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following compounds is NOT soluble in water?
A
K2SO4
B
NH4Br
C
NaNO3
D
AgCl
Verified step by step guidance1
Step 1: Understand the concept of solubility in water. Solubility depends on the ability of a compound to dissociate into ions and interact with water molecules through ion-dipole forces.
Step 2: Recall the general solubility rules for ionic compounds in water: most alkali metal salts (like K+, Na+) and ammonium (NH4+) salts are soluble, as well as most nitrates (NO3-) and sulfates (SO4^2-), with some exceptions.
Step 3: Analyze each compound given: K2SO4 contains potassium and sulfate ions, both generally soluble; NH4Br contains ammonium and bromide ions, both soluble; NaNO3 contains sodium and nitrate ions, both soluble.
Step 4: Recognize that AgCl (silver chloride) is a well-known exception to solubility rules, as most silver salts are poorly soluble in water due to the strong ionic lattice and low hydration energy.
Step 5: Conclude that among the listed compounds, AgCl is the one that is NOT soluble in water, based on solubility rules and exceptions.
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