strong dissolved electrolytes
💧ACS GENERAL CHEMISTRY STUDY GUIDE
Aqueous Reactions and Solubility for the ACS Exam
Review electrolytes, net ionic equations, precipitation, titration, solubility products, and common-ion calculations.
8 key ideas8 flashcards5 practice questions
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Split, cancel, and keep only what reacts.
solids, liquids, gases, weak species
spectator ions on both sides
Key ideas to know
Start with the relationships between ideas. Then close the notes and explain each one from memory.
- 01
Strong electrolytes separate nearly fully into ions in water.
- 02
A net ionic equation removes spectator ions that appear unchanged on both sides.
- 03
A precipitation reaction forms a sparingly soluble solid from dissolved ions.
- 04
Solubility rules help predict whether an ionic compound remains dissolved.
- 05
The ion product Q is compared with Ksp to predict precipitation.
- 06
Molar solubility must be connected to ion concentrations through dissolution stoichiometry.
- 07
A common ion lowers the solubility of a sparingly soluble salt at equilibrium.
- 08
Selective precipitation depends on differing ion concentrations and solubility-product thresholds.
PART OF THE ACS GENERAL CHEMISTRY GUIDE
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Open the full ACS General Chemistry guide →Two ideas worth correcting now
NOT QUITE
→All ionic compounds dissolve fully in water
USE THIS INSTEAD
Many ionic solids have limited solubility.
NOT QUITE
→A saturated solution contains no dissolved solid
USE THIS INSTEAD
It contains the equilibrium dissolved concentration while undissolved solid may remain.
Flashcards
Answer before opening each card. The effort to retrieve is part of the learning.
1What is a spectator ion?Show answer ＋
An ion present in the same form before and after a reaction.
2What is a net ionic equation?Show answer ＋
An equation containing only species that undergo reaction.
3When does precipitation begin?Show answer ＋
When the ion product exceeds the solubility product under the stated conditions.
4What does Ksp describe?Show answer ＋
The equilibrium constant for dissolution of a sparingly soluble ionic solid.
5Does a larger Ksp always mean greater molar solubility?Show answer ＋
Not without checking dissolution stoichiometry.
6What is the common-ion effect?Show answer ＋
Reduced dissolution when a dissolved ion is already present.
7Why are pure solids absent from Ksp expressions?Show answer ＋
Their activity is treated as constant.
8What is an equivalence point in a titration?Show answer ＋
The point where stoichiometric amounts of analyte and titrant have reacted.
Explain it in your own words
Use the answer as a check after you have written or spoken your response.
01How is a complete ionic equation converted to a net ionic equation?
Split strong aqueous electrolytes into ions, retain solids, liquids, gases, and weak electrolytes, then cancel unchanged ions.
02Will silver chloride precipitate after mixing two solutions?
Calculate the post-mixing silver and chloride concentrations, multiply them, and compare Q with Ksp.
03Why can dilution prevent precipitation?
Mixing lowers ion concentrations, which can keep Q below Ksp.
04How do you relate CaF2 molar solubility s to ion concentrations?
Calcium concentration is s and fluoride concentration is 2s, so Ksp equals s times 2s squared.
05Why can selective precipitation separate ions?
One salt reaches its Ksp threshold at a lower reagent concentration than another.
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