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Acids bases and salts-Key Points

Acids, Bases and Salts

Key Concepts

1. Conjugate Acid of a Base

The positively charged ion formed when a base accepts a proton is called its conjugate acid.

2. Conjugate Base of an Acid

The species that remains after an acid donates a proton is its conjugate base.

3. Bronsted-Lowry Theory

Acids: Proton donors
Bases: Proton acceptors

4. pH of a Solution

pH is the negative logarithm of the hydrogen ion concentration: pH = -log[H⁺]

5. pKw

pKw is the negative logarithm of the ionization constant of water.

6. Leveling Effect

Strong acids or bases show similar strengths in water due to the solvent's leveling property.

7. Buffer Solution

A buffer resists changes in pH when small amounts of acid or base are added.

8. Acid-Base Indicator

A weak acid or base that changes color in response to pH changes in a solution.

9. Titration

A laboratory method used to determine the concentration of an unknown solution by neutralization.

10. pKa

The negative logarithm of the acid dissociation constant (Ka): pKa = -log(Ka)

11. pKb

The negative logarithm of the base dissociation constant (Kb): pKb = -log(Kb)

12. Lewis Acid-Base Concept

Acid: Electron pair acceptor
Base: Electron pair donor

13. Buffer Action

The ability of a buffer to maintain its pH even when small amounts of acids or bases are added.

14. Buffer Capacity

The measure of a buffer’s ability to resist pH changes.

15. Hydrolysis

The reaction of salt ions with water to form acidic or basic solutions.

16. Leveling Effect (Revisited)

The equalization of the strength of strong acids and bases in a given solvent due to complete ionization.

Study Tip 💡

Memorize the definitions and differences between various acid-base concepts (Bronsted-Lowry vs. Lewis) to strengthen your conceptual understanding for exams.

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