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Understanding Acids and Bases: Properties, Reactions, and Definitions

Explore the characteristics and behaviors of acids and bases, including their tastes, reactions, and roles as electrolytes. Discover the pH scale, the Arrhenius and Brønsted-Lowry theories, and how acids and bases neutralize each other. Learn about examples such as hydrochloric acid and sodium hydroxide, along with the concept of conjugate acids and bases. Find out how water can act as both an acid and a base, and delve into important calculations for neutralization reactions. This comprehensive overview equips you with a foundational understanding of these essential chemical concepts.

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Understanding Acids and Bases: Properties, Reactions, and Definitions

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  1. ACIDS AND BASES

  2. Characteristics of Acids • Taste Sour • React with metals • Electrolytes (conduct electricity) • Affect indicators (red=acid) • Neutralize Bases • pH between 0 and <7

  3. Characteristics of Bases • Taste Bitter • Feel Slippery • Electrolytes (conduct electricity) • Neutralize Acids (Antacids) • Affect indicators (base=blue) • pH between >7 and 14

  4. Examples of Acids • HCl monoprotic • H2SO4diprotic • H3PO4 triprotic • HNO3

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

  6. There are 2 definitions for acids and bases • Arrhenius Theory • Brønsted-Lowry Theory

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

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

  9. 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

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

  11. So who is the Arrhenius Acid given: H2SO4 + H2O  H3O+ + HSO4- H2SO4 Why? Because it produces H+

  12. So who is the Arrhenius Base given: NaOH + H2O  Na+ + OH- + H2O NaOH Why? Because it produces OH-

  13. The world was cool with the Arrehenius definition until NH3 (Ammonia) came along. When combined with water it did not make OH- ions…looks like we need a new definition.

  14. Brønsted-Lowry Theory ON ACIDS…Acids are substances that are capable of donating a proton (H+)

  15. Brønsted-Lowry Theory ON BASES…Bases are substances that are capable of accepting a proton (H+)

  16. Example of 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.

  17. Example of 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.

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

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

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

  21. What is pH? A measurement of the concentration of H3O+ ions (H+ ions)

  22. pH Scale

  23. What is pH? Kw = [H+][OH-] = 1 x 10-14 pH = -log[H+] pOH = -log[OH-]

  24. pH Scale

  25. Neutralization of Bases using Acids

  26. Neutralization acid base nMV = nMV

  27. How many milliliters of 0.80 M HCl are needed to neutralize 35 mL of 1.5 M NaOH? HCl + NaOH  NaCl + H2O 66 mL

  28. What is the concentration of a solution of H2SO4 if it takes 35 mL to neutralize 55 mL of 1.5 M Mg(OH)2? H2SO4 + Mg(OH)2 MgSO4 + 2 H2O 2.4M

  29. How many milliliters of 1.8 M HCl are needed to neutralize 85 mL of 1.0 M NaOH? HCl + NaOH  NaCl + H2O 47 mL

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

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

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

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

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