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Understanding Acids and Bases: Key Differences and Definitions

Explore the distinct properties and definitions of acids and bases in chemistry. Acidic solutions feature a higher concentration of hydrogen ions (H+) than hydroxide ions (OH-), while basic solutions have the opposite. Water is considered neutral, containing equal amounts of both ions. Discover key acid-base theories, including Arrhenius and Brønsted-Lowry definitions, the concept of conjugate acid-base pairs, and the role of amphoteric substances. Gain insights into polyprotic acids, which can donate multiple hydrogen ions sequentially.

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Understanding Acids and Bases: Key Differences and Definitions

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  1. Acids and Bases…What’s the difference?

  2. Acid vs Base • Acidic Solutions-contain more hydrogen ions (H+) than hydroxide ions (OH-) • Basic solutions contain more hydroxide ions than hydrogen ions

  3. Water=Neutral • There are equal amounts of hydrogen ions as hydroxide ions • Note: H3O+ is the same as H+

  4. Arrhenius Acid • A substance ionizes and produces hydrogen ions

  5. Arrhenius Base • A substance that ionizes to produce hydroxide ions

  6. Brønsted-Lowry Acid • An acid is something that donates a hydrogen • An acid is something that accepts a hydrogen

  7. Brønsted-Lowry Acid

  8. Brønsted-Lowry Conjugate Acids and Bases • Conjugate Acid: the species produced when a base accepts a hydrogen • Conjugate Base: the species produced when an acid donates a base

  9. Brønsted-Lowry Conjugate Acids and Bases

  10. Brønsted-Lowry Conjugate Acids and Bases

  11. Amphoteric Substances • Water (and other species) that can act as acids or bases

  12. Identify the conjugate acid/base pairs

  13. Polyprotic Acids • When an acid donates more than one hydrogen-one is lost at a time!

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