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 type of salts will generally be more soluble in an acidic solution than in pure water?

Salts containing anions of weak acids, such as carbonates (CO_3^{2-}) and phosphates (PO_4^{3-})

Salts containing halide anions, such as Cl^- and Br^-

Salts containing nitrate anions (NO_3^-)

Salts containing alkali metal cations, such as Na^+ and K^+

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Verified step by step guidance

Step 1: Understand that the solubility of salts in water can be influenced by the pH of the solution, especially if the salt contains anions that can react with H\textsuperscript{+} ions (protons) from an acid.

Step 2: Identify that salts containing anions of weak acids (like CO\_3\^{2-} from carbonic acid and PO\_4\^{3-} from phosphoric acid) can react with H\textsuperscript{+} ions in acidic solution, forming their corresponding weak acids and thus reducing the concentration of free anions.

Step 3: Recognize that this reaction shifts the dissolution equilibrium of the salt to dissolve more solid to replace the consumed anions, effectively increasing the salt's solubility in acidic solution compared to pure water.

Step 4: Contrast this with salts containing anions of strong acids (like NO\_3\^- from nitric acid) or halide ions (Cl\^-, Br\^-), which do not react significantly with H\textsuperscript{+} ions, so their solubility remains largely unchanged in acidic conditions.

Step 5: Conclude that salts containing anions of weak acids are generally more soluble in acidic solutions than in pure water due to the acid-base reaction that consumes the anions and drives dissolution.