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

Which of the following solutions will form a precipitate when mixed with a solution of aqueous Na2CO3?

CaCl2(aq)

KNO3(aq)

NaCl(aq)

Li2SO4(aq)

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Verified step by step guidance

Identify the ions present in the aqueous sodium carbonate (Na2CO3) solution. It dissociates into 2 Na\textsuperscript{+} ions and 1 CO\textsubscript{3}\textsuperscript{2-} ion.

For each given solution, write down the ions it dissociates into when dissolved in water: CaCl\textsubscript{2} \rightarrow Ca\textsuperscript{2+} and 2 Cl\textsuperscript{-}; KNO\textsubscript{3} \rightarrow K\textsuperscript{+} and NO\textsubscript{3}\textsuperscript{-}; NaCl \rightarrow Na\textsuperscript{+} and Cl\textsuperscript{-}; Li\textsubscript{2}SO\textsubscript{4} \rightarrow 2 Li\textsuperscript{+} and SO\textsubscript{4}\textsuperscript{2-}.

Consider the possible combinations of cations and anions from Na2CO3 and each salt to see if any insoluble compound (precipitate) can form. Use solubility rules to determine if a precipitate forms. For example, carbonate salts of Ca\textsuperscript{2+} are generally insoluble.

Check the solubility rules: most carbonates (CO\textsubscript{3}\textsuperscript{2-}) are insoluble except those of alkali metals (like Na\textsuperscript{+}, K\textsuperscript{+}, Li\textsuperscript{+}) and ammonium. Since CaCO\textsubscript{3} is insoluble, mixing CaCl\textsubscript{2} with Na2CO3 will form a precipitate of CaCO\textsubscript{3}.

Conclude that only the mixture of CaCl\textsubscript{2} and Na2CO3 will form a precipitate, while the others remain soluble due to the solubility of their respective ions with carbonate.