Multiple Choice
Which of the following best describes a saturated solution?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following reactions will produce a precipitate? Select the reaction where a solid forms as a result of mixing the solutions.
A
Mixing NaCl(aq) and KNO3(aq) produces no precipitate.
B
Mixing NH4Cl(aq) and NaNO3(aq) produces no precipitate.
C
Mixing KNO3(aq) and Na2SO4(aq) produces no visible change.
D
Mixing NaCl(aq) and AgNO3(aq) produces a white solid.
Verified step by step guidance1
Step 1: Understand that a precipitate forms when two aqueous solutions are mixed and an insoluble solid product is formed due to a double displacement reaction.
Step 2: Identify the ions present in each solution for the given reactions. For example, NaCl(aq) contains Na⁺ and Cl⁻ ions, and AgNO3(aq) contains Ag⁺ and NO3⁻ ions.
Step 3: Use solubility rules to determine if any combination of cations and anions from the mixed solutions forms an insoluble compound. For instance, most nitrates (NO3⁻) are soluble, but silver chloride (AgCl) is insoluble and forms a precipitate.
Step 4: Analyze each reaction: mixing NaCl and KNO3 produces only soluble ions (Na⁺, K⁺, Cl⁻, NO3⁻), so no precipitate forms; similarly, NH4Cl and NaNO3 produce only soluble ions; KNO3 and Na2SO4 also produce only soluble ions.
Step 5: Conclude that mixing NaCl and AgNO3 results in the formation of AgCl, a white solid precipitate, because AgCl is insoluble in water according to solubility rules.
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