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Properties of Acids and Bases

Properties of Acids and Bases. Acids taste sour, will change the color of an acid base indicator, and can be strong or weak electrolytes in aqueous solution. Properties of Acids and Bases.

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Properties of Acids and Bases

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  1. Properties of Acids and Bases Acids taste sour, will change the color of an acid base indicator, and can be strong or weak electrolytes in aqueous solution.

  2. Properties of Acids and Bases Bases taste bitter, feel slippery, will change the color of an acid-base indicator, and can be strong or weak electrolytes in aqueous solution.

  3. Arrhenius Acids and Bases Arrhenius acids are compounds that ionize to yield hydrogen ions (H+) in aqueous solution.

  4. Arrhenius Acids and Bases An Arrhenius base is a compound that ionizes to yield hydroxide ions (OH-) in aqueous solution.

  5. Bronsted-Lowry Acids and Bases The Bronsted-Lowry theory defines an acid as a hydrogen-ion donor and a base as a hydrogen-ion acceptor.

  6. Bronsted-Lowry Acids and Bases A conjugate acid is the particle formed when a base gains a hydrogen ion. A conjugate base is the particle formed when an acid has donated a hydrogen ion.

  7. Bronsted-Lowry Acids and Bases A conjugate acid-base pair consists of two substances related by the loss or gain of a single hydrogen ion.

  8. Bronsted-Lowry Acids and Bases

  9. Bronsted-Lowry Acids and Bases A water molecule that gains a hydrogen ion becomes a positively charged hydronium ion (H3O+). A substance that can act as both an acid and a base is said to be amphoteric.

  10. Lewis Acids and Bases A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. A Lewis base is a substance that can donate a pair of electrons to form a covalent bond.

  11. Acids and Bases

  12. Hydrogen Ions from Water

  13. Ion Product Constant for Water The product of the concentrations of the hydrogen ions and hydroxide ions in water is called the ion-product constant for water (Kw).

  14. Ion Product Constant for Water If [H+] = [OH-], then the solution is neutral. If [H+] > [OH-], then the solution is acidic. If [H+] < [OH-], then the solution is basic.

  15. The pH Concept In a neutral solution, the [H+] = 1 x 10-7M. The pH of a neutral solution is 7.

  16. The pH Concept If [H+] = [OH-], then the pH = 7. If [H+] > [OH-], then the pH < 7. If [H+] < [OH-], then the pH > 7.

  17. The pH Concept

  18. The pH Concept

  19. The pH Concept

  20. Measuring pH An indicator is a valuable tool for measuring pH because its acid form and base form have different colors in solution. Phenolphthalein changes from colorless to pink at pH 7-9.

  21. Measuring pH

  22. Strong and Weak Acids and Bases In general, strong acids are completely ionized in aqueous solution. Weak acids ionize only slightly in aqueous solution.

  23. Strong and Weak Acids and Bases Strong bases dissociate completely into metal ions and hydroxide ions in aqueous solution. Weak bases react with water to form the hydroxide ion and the conjugate acid of the base.

  24. Strong and Weak Acids and Bases

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