Multiple Choice
How does increasing the amount of sugar in a supersaturated solution affect the likelihood of crystallization occurring?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following compounds is most soluble in water?
A
AgCl
B
PbBr_2
C
NaNO_3
D
BaSO_4
Verified step by step guidance1
Step 1: Understand that solubility in water depends largely on the compound's ability to dissociate into ions and the lattice energy of the solid versus the hydration energy of the ions.
Step 2: Recognize that ionic compounds containing alkali metal ions (like Na⁺) and nitrate ions (NO₃⁻) are generally very soluble in water due to strong ion-dipole interactions with water molecules.
Step 3: Compare the given compounds: AgCl, PbBr₂, BaSO₄ are all salts with ions that tend to form less soluble compounds because of higher lattice energies and lower hydration energies relative to NaNO₃.
Step 4: Recall the solubility rules: nitrates (NO₃⁻) are typically soluble with no common exceptions, while chlorides, bromides, and sulfates have varying solubilities and often form precipitates with certain cations.
Step 5: Conclude that NaNO₃ is the most soluble compound among the options because it fully dissociates in water and does not form a precipitate, unlike the other salts listed.
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