Multiple Choice
Which of the following compounds is soluble in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following salts would have the lowest solubility in water?
A
NH4Br
B
K2SO4
C
NaNO3
D
AgCl
Verified step by step guidance1
Identify the salts given in the problem and note their common ions: NH4Br (ammonium bromide), K2SO4 (potassium sulfate), NaNO3 (sodium nitrate), and AgCl (silver chloride).
Recall that solubility in water depends on the nature of the salt, particularly the lattice energy and the hydration energy of the ions, as well as the solubility product constant (K\_sp) for slightly soluble salts.
Recognize that NH4Br, K2SO4, and NaNO3 are generally highly soluble ionic salts because they contain alkali metal or ammonium ions paired with common anions, which typically have high solubility in water.
Understand that AgCl is a salt known for its low solubility in water due to its very low solubility product constant (K\_sp), meaning it dissociates very little in aqueous solution.
Conclude that among the given options, AgCl has the lowest solubility in water because it is a classic example of a sparingly soluble salt, unlike the other salts which are highly soluble.
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