Multiple Choice
Which of the following ions will form a precipitate when mixed with Pb^{2+} (lead(II) cation) in aqueous solution?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following compounds is expected to be the most soluble in H2O?
A
CaCO3
B
NaNO3
C
BaSO4
D
AgCl
Verified step by step guidance1
Step 1: Understand that solubility in water depends on the compound's ability to dissociate into ions and the lattice energy of the solid versus the hydration energy of the ions formed.
Step 2: Recognize that ionic compounds with highly soluble ions (like Na+ and NO3-) tend to be more soluble in water because the hydration energy overcomes the lattice energy.
Step 3: Recall common solubility rules: nitrates (NO3-) are generally soluble in water, while carbonates (CO3^2-), sulfates (SO4^2-), and chlorides (Cl-) have varying solubilities depending on the cation.
Step 4: Compare the given compounds: CaCO3, BaSO4, and AgCl are known to be sparingly soluble or insoluble in water, while NaNO3 is highly soluble due to the nitrate ion.
Step 5: Conclude that NaNO3 is expected to be the most soluble in water because it contains the nitrate ion, which forms compounds that are generally very soluble.
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