In the crystal observatories of the sky-realm Zephyrus, an arcane botanist must prepare a mineral irrigation blend that remains entirely clear to avoid clogging delicate nutrient conduits. The botanist tests four separate combinations of clear, equimolar aqueous solutions to find one that produces no precipitate upon mixing. Based on general solubility rules, which pair of aqueous solutions will remain completely free of a solid precipitate when combined?

A) $\text{KNO}_3\text{(aq)}$ and $\text{CuCl}_2\text{(aq)}$

B) $\text{Pb(NO}_3\text{)}_2\text{(aq)}$ and $\text{KI(aq)}$

C) $\text{BaCl}_2\text{(aq)}$ and $\text{Na}_2\text{SO}_4\text{(aq)}$

D) $\text{Ca(NO}_3\text{)}_2\text{(aq)}$ and $\text{Li}_3\text{PO}_4\text{(aq)}$

Deep within the bioluminescent crystal towers of the planet Zephyria, an environmental alchemist treats a mineral runoff containing equal concentrations of dissolved barium nitrate, $\text{Ba(NO}_3\text{)}_2$, and magnesium nitrate, $\text{Mg(NO}_3\text{)}_2$. The alchemist must selectively precipitate the barium ions as a solid salt while keeping all magnesium ions dissolved in the aqueous phase. Based on general solubility rules, which reagent should be added to achieve this selective precipitation?

A) Sodium carbonate, $\text{Na}_2\text{CO}_3$, because carbonate anions precipitate barium ions while keeping magnesium ions dissolved.

B) Potassium hydroxide, $\text{KOH}$, because hydroxide anions precipitate barium ions while magnesium hydroxide is completely soluble.

C) Sodium sulfate, $\text{Na}_2\text{SO}_4$, because barium sulfate is insoluble in water whereas magnesium sulfate remains soluble.

D) Ammonium nitrate, $\text{NH}_4\text{NO}_3$, because nitrate anions form an insoluble precipitate specifically with heavy alkaline earth cations.

In the crystal laboratories of the floating sky-city Aethelgard, an alchemical engineer purifies a wastewater reservoir containing dissolved nickel(II) sulfate, $\text{NiSO}_4$, by blending it with an aqueous solution of potassium hydroxide, $\text{KOH}$. A vibrant green solid immediately forms and settles to the bottom of the reaction vessel. Based on standard solubility rules, which statement correctly identifies the precipitate and the balanced net ionic equation for this reaction?

A) The precipitate is $\text{K}_2\text{SO}_4$, and the net ionic equation is $2\text{K}^+(aq) + \text{SO}_4^{2-}(aq) \rightarrow \text{K}_2\text{SO}_4(s)$.

B) The precipitate is $\text{Ni(OH)}_2$, and the net ionic equation is $\text{Ni}^{2+}(aq) + 2\text{OH}^-(aq) \rightarrow \text{Ni(OH)}_2(s)$.

C) The precipitate is $\text{Ni(OH)}_2$, and the net ionic equation is $\text{NiSO}_4(aq) + 2\text{KOH}(aq) \rightarrow \text{Ni(OH)}_2(s) + \text{K}_2\text{SO}_4(aq)$.

D) The precipitate is $\text{Ni(OH)}_2$, and the net ionic equation is $\text{Ni}^{2+}(aq) + \text{OH}^-(aq) \rightarrow \text{NiOH}(s)$.

During an expedition through the glowing subterranean caverns of Mount Lumina, explorers collect a mineral drainage stream containing dissolved silver nitrate, $ \text{AgNO}_3 $. To recover the precious silver before purifying the cavern's water source, the team treats the stream with an aqueous solution of calcium chloride, $ \text{CaCl}_2 $, immediately forming a dense white precipitate. Based on standard solubility rules, which statement correctly identifies the precipitate formed and the spectator ions remaining dissolved in the water?

A) The precipitate is $ \text{Ca(NO}_3)_2 $, and the spectator ions are $ \text{Ag}^+ $ and $ \text{Cl}^- $.

B) The precipitate is $ \text{AgCl} $, and the spectator ions are $ \text{Ag}^+ $ and $ \text{NO}_3^- $.

C) The precipitate is $ \text{Ca(NO}_3)_2 $, and the spectator ions are $ \text{Ca}^{2+} $ and $ \text{Cl}^- $.

D) The precipitate is $ \text{AgCl} $, and the spectator ions are $ \text{Ca}^{2+} $ and $ \text{NO}_3^- $.

Precipitation reactions and solubility rules Original Scenario-Based Practice

Chemistry · The Mole & Stoichiometry · Chemistry · Chemical Reactions & Equations

5 Chemistry practice questions on Precipitation reactions and solubility rules. Questions built around original scenarios.

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1.
In the floating atmospheric conservatory of Cloud-Spire Zenith, an environmental alchemist synthesizes phosphorescent mineral seeds by combining an aqueous solution containing 0.200 mol of sodium phosphate, $\text{Na}_3\text{PO}_4$ , with an aqueous solution containing 0.240 mol of calcium chloride, $\text{CaCl}_2$ . Based on solubility rules and reaction stoichiometry, what is the maximum amount of solid precipitate that can form from this mixture?
- A) 0.100 mol
- B) 0.080 mol
- C) 0.120 mol
- D) 0.240 mol
2.
In the crystal observatories of the sky-realm Zephyrus, an arcane botanist must prepare a mineral irrigation blend that remains entirely clear to avoid clogging delicate nutrient conduits. The botanist tests four separate combinations of clear, equimolar aqueous solutions to find one that produces no precipitate upon mixing. Based on general solubility rules, which pair of aqueous solutions will remain completely free of a solid precipitate when combined?
- A) $\text{KNO}_3\text{(aq)}$ and $\text{CuCl}_2\text{(aq)}$
- B) $\text{Pb(NO}_3\text{)}_2\text{(aq)}$ and $\text{KI(aq)}$
- C) $\text{BaCl}_2\text{(aq)}$ and $\text{Na}_2\text{SO}_4\text{(aq)}$
- D) $\text{Ca(NO}_3\text{)}_2\text{(aq)}$ and $\text{Li}_3\text{PO}_4\text{(aq)}$
3.
Deep within the bioluminescent crystal towers of the planet Zephyria, an environmental alchemist treats a mineral runoff containing equal concentrations of dissolved barium nitrate, $\text{Ba(NO}_3\text{)}_2$ , and magnesium nitrate, $\text{Mg(NO}_3\text{)}_2$ . The alchemist must selectively precipitate the barium ions as a solid salt while keeping all magnesium ions dissolved in the aqueous phase. Based on general solubility rules, which reagent should be added to achieve this selective precipitation?
- A) Sodium carbonate, $\text{Na}_2\text{CO}_3$ , because carbonate anions precipitate barium ions while keeping magnesium ions dissolved.
- B) Potassium hydroxide, $\text{KOH}$ , because hydroxide anions precipitate barium ions while magnesium hydroxide is completely soluble.
- C) Sodium sulfate, $\text{Na}_2\text{SO}_4$ , because barium sulfate is insoluble in water whereas magnesium sulfate remains soluble.
- D) Ammonium nitrate, $\text{NH}_4\text{NO}_3$ , because nitrate anions form an insoluble precipitate specifically with heavy alkaline earth cations.
4.
In the crystal laboratories of the floating sky-city Aethelgard, an alchemical engineer purifies a wastewater reservoir containing dissolved nickel(II) sulfate, $\text{NiSO}_4$ , by blending it with an aqueous solution of potassium hydroxide, $\text{KOH}$ . A vibrant green solid immediately forms and settles to the bottom of the reaction vessel. Based on standard solubility rules, which statement correctly identifies the precipitate and the balanced net ionic equation for this reaction?
- A) The precipitate is $\text{K}_2\text{SO}_4$ , and the net ionic equation is $2\text{K}^+(aq) + \text{SO}_4^{2-}(aq) \rightarrow \text{K}_2\text{SO}_4(s)$ .
- B) The precipitate is $\text{Ni(OH)}_2$ , and the net ionic equation is $\text{Ni}^{2+}(aq) + 2\text{OH}^-(aq) \rightarrow \text{Ni(OH)}_2(s)$ .
- C) The precipitate is $\text{Ni(OH)}_2$ , and the net ionic equation is $\text{NiSO}_4(aq) + 2\text{KOH}(aq) \rightarrow \text{Ni(OH)}_2(s) + \text{K}_2\text{SO}_4(aq)$ .
- D) The precipitate is $\text{Ni(OH)}_2$ , and the net ionic equation is $\text{Ni}^{2+}(aq) + \text{OH}^-(aq) \rightarrow \text{NiOH}(s)$ .
5.
During an expedition through the glowing subterranean caverns of Mount Lumina, explorers collect a mineral drainage stream containing dissolved silver nitrate, $\text{AgNO}_3$ . To recover the precious silver before purifying the cavern's water source, the team treats the stream with an aqueous solution of calcium chloride, $\text{CaCl}_2$ , immediately forming a dense white precipitate. Based on standard solubility rules, which statement correctly identifies the precipitate formed and the spectator ions remaining dissolved in the water?
- A) The precipitate is $\text{Ca(NO}_3)_2$ , and the spectator ions are $\text{Ag}^+$ and $\text{Cl}^-$ .
- B) The precipitate is $\text{AgCl}$ , and the spectator ions are $\text{Ag}^+$ and $\text{NO}_3^-$ .
- C) The precipitate is $\text{Ca(NO}_3)_2$ , and the spectator ions are $\text{Ca}^{2+}$ and $\text{Cl}^-$ .
- D) The precipitate is $\text{AgCl}$ , and the spectator ions are $\text{Ca}^{2+}$ and $\text{NO}_3^-$ .

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