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ACIDS y BASES

ACIDS y BASES. Characteristics of Acids. Taste Sour Affect indicators (red=acid) Neutralize Bases Often produce hydrogen gas pH between 0 and <7. Characteristics of Bases. Taste Bitter Feel Slippery Neutralize Acids (Antacids) Affect indicators (base=blue) pH between >7 and 14

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ACIDS y BASES

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  1. ACIDS y BASES

  2. Characteristics of Acids • Taste Sour • Affect indicators (red=acid) • Neutralize Bases • Often produce hydrogen gas • pH between 0 and <7

  3. Characteristics of Bases • Taste Bitter • Feel Slippery • Neutralize Acids (Antacids) • Affect indicators (base=blue) • pH between >7 and 14 • Dissolve grease (Drano, Windex)

  4. Examples of Acids • HCl • H2SO4 • HNO3 • HF • Juices

  5. Examples of Bases • NaOH • Ca(OH)2 • KOH • Soap, Ammonia, Lye, Baking Soda

  6. There are 3 definitions for acids and bases • Arrhenius Theory • Brønsted-Lowry Theory • Lewis Theory

  7. pH Scale

  8. pH Scale

  9. pH Scale

  10. pH Scale

  11. Arrehenius Theory ON ACIDS…An acid is a substance that ionizes in water to give hydrogen ions (H+)

  12. Arrehenius Theory ON BASES…A base is a substance that ionizes in water to give hydroxide ions (OH-)

  13. An example of the reaction of Hydrochloric Acid: HCl + H2O H3O+ + Cl- When the HCl breaks apart the free H+is attracted to the H2O and forms a HYDRONIUM ION

  14. So who is the Arrhenius Acid given: HCl + H2O H3O+ + Cl- HCl Why? Because it produces H+

  15. An example of the reaction of Potassium Hydroxide: KOH + H2O K+ + 2OH- When the KOH breaks apart it forms the HYDROXIDE ION (OH-)

  16. So who is the Arrhenius Base given: KOH + H2O K+ + 2OH- KOH Why? Because it produces OH-

  17. The world was cool with the Arrehenius definition until NH3 (Ammonia) came along.When combined with water it increased the number of OH- ions…looks like we need a new definition

  18. Brønsted-Lowry Theory ON ACIDS…Acids are substances that are capable of donating a proton

  19. Brønsted-Lowry Theory ON BASES…Bases are substances capable of accepting a proton

  20. Example Brønsted Acids and Bases: NH3 + H2O  NH4+ + OH- Here, H2O acts as a Brønsted acid by donating a proton to NH3 which acts as a Brønsted base.

  21. Example Brønsted Acids and Bases: NH4+ + OH-NH3 + H2O In this case, NH4+ acts as an acid which donates a proton to OH-. OH- acts as a base.

  22. Lewis Theory ON ACIDS…Acids are substances that are electron-pair receptors

  23. Lewis Theory ON BASES…Bases are substances capable of donating electron-pairs

  24. Conjugate Base The substance that remains after an acid has donated a H+ ion

  25. Conjugate Acid The substance formed when a base accepts a H+ ion

  26. Conjugate Acids and Base NH3 + H2O NH4+ + OH- NH4+ + OH-NH3 + H2O For example, NH4+ is the conjugate acid of NH3 (1stequation), and NH3 is the conjugate base of NH4+ (2nd equation).

  27. Interesting fact… Water can act as an acid or a base!!!

  28. Amphoteric A substance that can act as either an acid or a base.

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