acids and bases power point presentation

Presentation about acids and bases

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 H 2 SO 4 HNO 3 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. ON ACIDS… An acid is a substance that ionizes in water to give hydrogen ions (H + ) Arrehenius Theory

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

13. An example of the reaction of Hydrochloric Acid: When the HCl breaks apart the free H + is attracted to the H 2 O and forms a HYDRONIUM ION HCl + H 2 O  H 3 O + + Cl -

14. So who is the Arrhenius Acid given: HCl HCl + H 2 O  H 3 O + + Cl - Why? Because it produces H +

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

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

17. The world was cool with the Arrehenius definition until NH 3 (Ammonia) came along. When combined with water it increased the number of OH - ions…looks like we need a new definition

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

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

20. Example Brønsted Acids and Bases: Here, H 2 O acts as a Brønsted acid by donating a proton to NH 3 which acts as a Brønsted base. NH 3 + H 2 O  NH 4 + + OH -

21. Example Brønsted Acids and Bases: In this case, NH 4 + acts as an acid which donates a proton to OH - . OH - acts as a base. NH 4 + + OH -  NH 3 + H 2 O

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

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

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

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

26. Conjugate Acids and Base For example, NH 4 + is the conjugate acid of NH 3 (1 st equation) , and NH 3 is the conjugate base of NH 4 + (2 nd equation) . NH 3 + H 2 O NH 4 + + OH - NH 4 + + OH -  NH 3 + H 2 O

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

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