Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

6. Chemical Quantities & Aqueous Reactions

Solubility Rules

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Solubility Rules

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Multiple Choice

A solution containing calcium nitrate is mixed with one containing potassium sulfate to form a solution that is 0.0100 M inCa(NO₃)₂ and 0.00250 M in K₂SO₄. Which of the following accurately describes what occurs when the new solution forms?

Calcium sulfate precipitates.

Potassium nitrate precipitates.

Both calcium sulfate and potassium nitrate precipitate.

No precipitate forms.

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Verified step by step guidance

Identify the possible products of the reaction between calcium nitrate \((\text{Ca(NO}_3\text{)}_2)\) and potassium sulfate \((\text{K}_2\text{SO}_4)\). The potential products are calcium sulfate \((\text{CaSO}_4)\) and potassium nitrate \((\text{KNO}_3)\).

Determine the solubility of the potential products. Calcium sulfate \((\text{CaSO}_4)\) is slightly soluble in water, while potassium nitrate \((\text{KNO}_3)\) is highly soluble.

Calculate the ion product \((Q)\) for calcium sulfate using the concentrations of calcium ions \((\text{Ca}^{2+})\) and sulfate ions \((\text{SO}_4^{2-})\) in the solution. Use the formula: \(Q = [\text{Ca}^{2+}][\text{SO}_4^{2-}]\).

Compare the ion product \((Q)\) to the solubility product constant \((K_{sp})\) of calcium sulfate. If \(Q > K_{sp}\), a precipitate will form. If \(Q \leq K_{sp}\), no precipitate will form.

Since potassium nitrate is highly soluble, it will not precipitate under normal conditions. Therefore, if \(Q \leq K_{sp}\) for calcium sulfate, no precipitate forms in the solution.