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Questions and Answers
What is the pH of a neutral solution?
What is the pH of a neutral solution?
7
What is the difference between a strong acid and a weak acid?
What is the difference between a strong acid and a weak acid?
A strong acid completely dissociates in water, while a weak acid partially dissociates in water.
What is a neutralization reaction, and what are the products of this reaction?
What is a neutralization reaction, and what are the products of this reaction?
A neutralization reaction is a reaction between an acid and a base, resulting in the formation of a salt and water.
What is the difference between a normal salt, an acid salt, and a basic salt?
What is the difference between a normal salt, an acid salt, and a basic salt?
What determines the solubility of a salt?
What determines the solubility of a salt?
What is a unique property of salts that allows them to conduct electricity?
What is a unique property of salts that allows them to conduct electricity?
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Study Notes
Acid-Base Chemistry
pH Scale
- pH: measure of hydrogen ion concentration
- pH 7: neutral (neither acidic nor basic)
- pH < 7: acidic
- pH > 7: basic
Acid-Base Reactions
- Acid (donates H+): HCl → H+ + Cl-
- Base (accepts H+): NaOH → Na+ + OH-
- Neutralization reaction: HCl + NaOH → NaCl + H2O
Strong and Weak Acids/Bases
- Strong acids: completely dissociate in water (e.g., HCl, HNO3)
- Weak acids: partially dissociate in water (e.g., CH3COOH)
- Strong bases: completely dissociate in water (e.g., NaOH, KOH)
- Weak bases: partially dissociate in water (e.g., NH3)
Salts
Formation of Salts
- Neutralization reaction: acid + base → salt + water
- Example: HCl + NaOH → NaCl (table salt) + H2O
Types of Salts
- Normal salts: contain only one type of cation and anion (e.g., NaCl)
- Acid salts: contain a cation and an anion from a weak acid (e.g., NaCH3COO)
- Basic salts: contain a cation and an anion from a weak base (e.g., NH4Cl)
- Double salts: contain two different cations and anions (e.g., KAl(SO4)2·12H2O)
Properties of Salts
- Solubility: varies depending on the salt
- Conductivity: salts dissociate into ions, allowing them to conduct electricity
Acid-Base Chemistry
pH Scale
- pH measures hydrogen ion concentration
- pH 7 is neutral (neither acidic nor basic)
- pH below 7 is acidic
- pH above 7 is basic
Acid-Base Reactions
- Acids donate H+ ions (e.g., HCl → H+ + Cl-)
- Bases accept H+ ions (e.g., NaOH → Na+ + OH-)
- Neutralization reaction: acid + base → salt + water (e.g., HCl + NaOH → NaCl + H2O)
Strong and Weak Acids/Bases
- Strong acids completely dissociate in water (e.g., HCl, HNO3)
- Weak acids partially dissociate in water (e.g., CH3COOH)
- Strong bases completely dissociate in water (e.g., NaOH, KOH)
- Weak bases partially dissociate in water (e.g., NH3)
Salts
Formation of Salts
- Neutralization reaction forms salts and water from acid and base reaction
- Example: HCl + NaOH → NaCl (table salt) + H2O
Types of Salts
- Normal salts contain one type of cation and anion (e.g., NaCl)
- Acid salts contain a cation and an anion from a weak acid (e.g., NaCH3COO)
- Basic salts contain a cation and an anion from a weak base (e.g., NH4Cl)
- Double salts contain two different cations and anions (e.g., KAl(SO4)2·12H2O)
Properties of Salts
- Solubility varies depending on the salt
- Salts dissociate into ions, allowing them to conduct electricity
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