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5B: Acids and Bases Chapters 5.6 and 16

5B: Acids and Bases Chapters 5.6 and 16. 5.6 - Naming Acids An acid is – any chemical formula that begins with H No oxygen in the formula: Hydro_______ ic acid (called binary acids because they have just 2 elements, one of which is Hydrogen) Example: HCl – HBr –

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5B: Acids and Bases Chapters 5.6 and 16

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  1. 5B: Acids and Bases Chapters 5.6 and 16

  2. 5.6 - Naming Acids • An acid is – any chemical formula that begins with H • No oxygen in the formula: Hydro_______ic acid (called binary acids because they have just 2 elements, one of which is Hydrogen) • Example: HCl – • HBr – • 2) Acid formed using “ate” polyatomic ion: ______ic acid • “Help! I ATE the ICky acid!” • Example: HNO3 – • H2SO4 – • 3) Acids formed using “ite” polyatomic ion: ________ous acid (Note that the “ite” ion has one less oxygen than the “ate” ion) • Example: HNO2 – • H2SO3 –

  3. 16.1 - Arrhenius • Acid- • HA→H+ + A- • Base- • BOH→B+ + OH- • This model is limited because it only allows for one kind of base.

  4. Characteristics

  5. Bronsted-Lowry Model- • Acid- • Base- • Conjugate acid-base pair- • HA + H2O → H3O+ + A- • A- + H2O → HA + OH- • Hydronium ion-

  6. 16.2 - Acid Strength • Strong Acids- • Weak Conjugate Base • Examples: • Weak Acids- • Strong Conjugate Base • Examples:

  7. Figure 16.1: Graphical representation of the behavior of acids of different strengths in aqueous solution.

  8. Diprotic Acid • Sulfuric Acid • Polyprotic Acid • Phosphoric Acid • Oxyacids • Organic acids (carboxyl group)

  9. Strong Bases • Use Your Solubility Rules

  10. 16.3 - Water as an Acid and Base • Amphoteric Species • Anything that has the ability to act as an acid or a base Examples:

  11. Aqueous Solutions • Acidic Solutions • [H+] > [OH-] • pH < 7 • Basic Solutions • [H+] < [OH-] • pH >7 • Neutral Solutions • [H+] = [OH-] • pH = 7

  12. 16.4 - The pH Scale pH= - log[H+] • see pg. 498 for how to use your calculator • Example 16.5 on pg. 499 pOH = -log[OH-] • Example 16.6 on pg. 500 • See pg. 500 for the pH scale and common substances

  13. pH + pOH = 14 • Calculating pOH from pH (see Example 16.7 on pg. 501) • Calculating pH from pOH • Calculating [H+] from pH (see Example 16.8 on pg. 503) • Calculating [OH-] from pOH (see Example 16.9 on pg. 503)

  14. 16.5 - Calculating the pH of Strong Acid and Base Solutions • Dissociation Equations 1.0 M HCl → 1.0 M H+ and 1.0 M Cl- 2.0 M NaOH→ 2.0 M Na+ and 2.0 M OH- • Problems (pg. 511, 55-58)

  15. 15.7 - Neutralization Reaction Stoichiometry • Neutralization Reaction is the reaction between an ACID and a BASE. • What are the products of a neutralization reaction?

  16. Net Ionic Equations for Strong-Strong Neutralization • HA + BOH → BA + HOH • H+ + A- + B+ + OH- → B+ + A- + HOH(l) • H+ + OH-→ HOH(l)

  17. How can we use a neutralization reaction and stoichiometry to calculate an unknown concentration?

  18. Titration • Using a solution of KNOWN concentration to determine the UNKNOWN concentration of another solution. • Titration calculations use MOLARITY and STOICHIOMETRY. MA VA = MBVB

  19. Indicators

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