객관식
Under what condition will a precipitate form in a solution when comparing the ion product (Q) to the solubility product constant (Ksp)?
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18. Aqueous Equilibrium
Precipitation: Ksp vs Q
객관식
Which of the following equations represents the precipitation reaction that occurs when solutions of ammonium chloride and iron(III) nitrate are mixed?
A
Fe(OH)3(s) forms as a precipitate.
B
FeCl3(s) forms as a precipitate.
C
No precipitation occurs.
D
NH4NO3(s) forms as a precipitate.
검증된 단계별 안내1
Identify the ions present in the solutions: Ammonium chloride (NH4Cl) dissociates into NH4^+ and Cl^- ions, while iron(III) nitrate (Fe(NO3)3) dissociates into Fe^3+ and NO3^- ions.
Consider the possible combinations of cations and anions that could form precipitates: NH4^+ with NO3^-, NH4^+ with Cl^-, Fe^3+ with Cl^-, and Fe^3+ with NO3^-.
Use solubility rules to determine which combinations could form a precipitate: Most nitrates (NO3^-) and ammonium (NH4^+) compounds are soluble, so NH4NO3 and NH4Cl are soluble. FeCl3 is also soluble in water.
Recognize that Fe^3+ can react with OH^- ions (from water or other sources) to form Fe(OH)3, which is insoluble and forms a precipitate.
Conclude that the precipitation reaction involves the formation of Fe(OH)3(s) as a precipitate when Fe^3+ ions react with OH^- ions in the solution.
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