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Weak Acids

Weak Acids. Acidity and Behavior, the Vinegar Example. Two forms of the acid exist in solution. Weak Acids Dissociate Poorly as Seen by Their Dissociation Constants, Ka. In other words, only one in a hundred protons dissociates!. And Its -log 10 , pK a. pKa = -log 10 K a

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Weak Acids

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  1. Weak Acids Acidity and Behavior, the Vinegar Example

  2. Two forms of the acid exist in solution

  3. Weak Acids Dissociate Poorly as Seen by Their Dissociation Constants, Ka In other words, only one in a hundred protons dissociates!

  4. And Its -log10, pKa • pKa = -log10Ka • Ka for acetic acid is 1.76 x 10-5M, • pKa = -log 1.76 x 10-5= ? • pKa for formic acid is 3.75, • Ka = 10-pKa= 10-3.75 = ?

  5. Table 1. Titration of 5% Acetic Acid With 1 M NaOH

  6. Figure 1. Titration of 5% Acetic Acid With 1 M NaOH

  7. Which Form Will Be Present? • Free acid form occurs at low pH • Conjugate base occurs at high pH • At some point amount of acid equals amount of base

  8. Henderson-Hasselbalch Equation

  9. Predicts the Ratio of Acid and Base, • What is the ratio of Ac- to HAc at pH 2.8? (See example on the right) • Practice: What is the ratio of Ac- to HAc at pH 6.8?

  10. but Not the pH • pKa is the pH where there are equal amounts of free acid and conjugate base • pH is dependent on the concentration of acid as well as its pKa • pKa ≠ pH of a solution, pH is usually <pKa The above formula is derived from the equilibrium constant equation assuming [H+] = [Ac-], and [HAc] >> [Ac-] The lower the pKa, the less valid the last assumption is.

  11. What’s going on at pKa? OrWhen does [HAc] = [Ac-]? When pH = pKa you can simplify the notation by representing the ratio with r, replace it in the equation, and solve its value. The ratio is 1 only when

  12. Landmarks on the titration curve Mostly Ac- Present [HAc] = [Ac-] pKa Mostly HAc Present

  13. Behavior of Vinegar Does not smell, can’t cross membranes pH of solution barely changes when base added Strong smell, crosses membranes

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