1 / 28

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

aikner
Download Presentation

ACIDS y BASES

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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.

More Related