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CHEM 5013 Applied Chemical Principles

CHEM 5013 Applied Chemical Principles. Acid / Base Chemistry Professor Bensley Alfred State College. Chapter Objectives. Recognize common strong acids and bases and common household acids and bases.

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CHEM 5013 Applied Chemical Principles

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  1. CHEM 5013 Applied Chemical Principles Acid / Base Chemistry Professor Bensley Alfred State College

  2. Chapter Objectives • Recognize common strong acids and bases and common household acids and bases. • Identify acids, bases and conjugate acid-base pairs according to the Bronsted-Lowry definitions.

  3. Chapter Objectives • Write molecular and ionic equations for acid-base neutralization reactions. • Understand the water ionization constant and realize how that is used to calculate pH, pOH, [H3O+], and [OH-]

  4. Acids and Bases • Acids: • Examples: • Bases: • Examples:

  5. Household Acids and Bases

  6. Brönsted-Lowry Concept • Acids: • Bases: H+ NH3 (aq) + H20 (l) NH4+ (aq) + OH- (aq) Base Acid H+ HNO3 (aq) + H20 (l) NO3- (aq) + H3O+ (aq) Acid Base

  7. Conjugate Acid – Base Pairs NH3 (aq) + H2O NH4+ (aq) + OH- (aq) BASE ACID CONJ. ACID CONJ. BASE OR NH3 (aq) + H2O NH4+ (aq) + OH- (aq) CONJ. BASE CONJ. ACID ACID BASE

  8. Example • Identify the acid and the base species in the following reaction: CO32- (aq) + H2O (l)  HCO3- (aq) + OH- (aq) • Label each species as an acid or base. Show the conjugate acid/base pairs. C2H3O2- (aq) + HNO2 (aq)  HC2H3O2 (aq) + NO2- (aq)

  9. Acid / Base Strengths • Strong acid: • Six main strong acids: HClO4 , H2SO4 , HI, HCl, HBr, HNO3 • Weak acid:

  10. Acid / Base Strengths • Strong base: • Six main strong bases: LiOH, NaOH, KOH, Ca(OH)2 , Sr(OH)2 , Ba(OH)2 Note: Group IA and IIA metals!!! • Weak base:

  11. Neutralization Reactions Acid + Base  Salt + Water 2HCl(aq) + Ca(OH)2(aq)  CaCl2(aq) + 2H2O(l)

  12. Water Ionization Constant • Kw= • What if I add a strong acid to water? 0.10M HCl in H2O  What is [H3O+]? What is [OH-]? • What if I add a strong base to water? 0.10M NaOH in H2O  What is [H3O+]? What is [OH-]?

  13. Example Calculate the [H3O+] and [OH-] at 25°C in 1.4 x 10-4 M Mg(OH)2 a strong base.

  14. Neutral, Acidic and Basic Solutions • Neutral solution: • Acidic solution: • Basic solution:

  15. pH Scale pH = [H3O+] = 0.1M pH = [H3O+] = 0.01M pH = [H3O+] = 0.001M pH =

  16. pH Scale • What is the pH of a neutral solution? • What is the pH of an acidic solution? • What is the pH of a basic solution? • Example What is the pH of typical adult blood where [H3O+] = 4.0x10-8 M

  17. pH Calculations pOH = pH + pOH = • Example: What is the pOH of typical adult blood?

  18. pH Calculations [H3O+] = • Typical adult blood has a pH of 7.40. What is [H3O+]?

  19. pH 1 2 3 4 5 6 7 8 9 10 11 Methyl Violet Phenolphthalein Bromthymol Blue Bromcresol Green Universal Indicator Methyl Orange [H3O+] 10-1 10-2 10-3 10-4 10-5 10-6 10-7 10-8 10-9 10-10 10-11

  20. Common Acids and Bases • Acids: • Hydrochloric Acid – • Sulfuric Acid – • Nitric Acid – • Acetic Acid – • Bases: • Sodium Hydroxide – • Ammonia –

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