Lecture 19.3- Weak vs. Strong HONORS
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Lecture 19.3- Weak vs. Strong HONORS

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Section 19.3 lecture for Honors Chem

Section 19.3 lecture for Honors Chem

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Lecture 19.3- Weak vs. Strong HONORS Lecture 19.3- Weak vs. Strong HONORS Presentation Transcript

  • BELLWORK- pH calcs Determine the pH of the following solutions. a) [H+] = 5.2x10-9 M b) [OH-] = 4.9x10-4 M c) pOH = 5.7 d) 0.02M HNO3 e) 0.10M NaOH
  • 19.3- Weak vs. Strong Lemons and grapefruits have a sour taste because they contain citric acid. Sulfuric acid is a widely used industrial chemical that can quickly cause severe burns if it comes into contact with skin. You will learn why some acids are weak and some acids are strong.
  • Strong acids and bases completely dissociate
  • Strong acids and bases completely dissociate AT EQUILIBRIUM HCl + H2O  Cl- + H3O+ little lots lots
  • Weak acids and bases only partly dissociate.
  • Weak acids and bases only partly dissociate. When in water most of the weak acid will keep its proton attached.
  • Weak acids and bases only partly dissociate. When in water most of the weak acid will keep its proton attached. Acetic acid(vinegar) is a weak acid.
  • Weak acids and bases only partly dissociate. When in water most of the weak acid will keep its proton attached. Acetic acid(vinegar) is a weak acid. AT EQUILIBRIUM CH3COOH + H2O  CH3COO- + H3O+ lots little little
  • Which acid will produce more H+, 1M HCl or 1M acetic acid?
  • Which acid will produce more H+, 1M HCl or 1M acetic acid? HCl is strong! HC2H3COO is weak
  • Recognize the name, formula, and relative strength (weak or strong) of the following: Memorize thisWEAK ACIDS STRONG ACIDS HCl hydrochloric acid CH3COOH H2SO4 sulfuric acid aka HC2H3O2 or HNO3 nitric acid acetic acid (vinegar) STRONG BASES WEAK BASES NaOH sodium hydroxide NH3 ammonia Bronsted-Lowry! KOH potassium hydroxide Arrhenius!
  • • A strong acid has a weak conjugate base. • A weak acid has a strong conjugate base. • A strong base has a weak conjugate acid. • A weak base has a strong conjugate acid.
  • Predict the products and label the conjugate acid-base pairs as weak or strong. NH3 + HCl  _______ + _______ CH3COOH + NH3  _______ + _______
  • An acid dissociation constant (Ka) describes the equilibrium between an acid and the ions it forms. HA H+ + A-
  • Weak acids have small Ka values. The stronger an acid is, the larger is its Ka value.
  • The base dissociation constant (Kb) describes the equilibrium of a base. [HB +][OH-] Kb = ---------------- [B] The larger the Kb the more dissociation occurs, so the stronger the base.