1 / 14

WEAK acids and bases in biochemistry…

The pH of a sample of blood is 7.4; the pH of a sample of gastric juice is 1.4. The blood sample has: A. 5.29 times lower [H+] than the gastric juice B. A million times higher [H+] than the gastric juice C. 6000 times lower [H+] than the gastric juice

ohuggins
Download Presentation

WEAK acids and bases in biochemistry…

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. The pH of a sample of blood is 7.4; the pH of a sample of gastric juice is 1.4. The blood sample has: A. 5.29 times lower [H+] than the gastric juice B. A million times higher [H+] than the gastric juice C. 6000 times lower [H+] than the gastric juice D. A million times lower [H+] than the gastric juice E. 0.189 times the [H+] as the gastric juice

  2. The pH of a sample of blood is 7.4; the pH of a sample of gastric juice is 1.4. The blood sample has: A. 5.29 times lower [H+] than the gastric juice B. A million times higher [H+] than the gastric juice C. 6000 times lower [H+] than the gastric juice D. A million times lower [H+] than the gastric juice * E. 0.189 times the [H+] as the gastric juice

  3. WEAK acids and bases in biochemistry… Tendency of an acid to dissociate HA<--> H+ + A- is described by Ka = ([H+][A-])/[HA] pKa = -log Ka (proton donor) (proton acceptor)

  4. WEAK acids and bases in biochemistry… Tendency of an acid to dissociate HA<-> H+ + A- is described by Ka = ([H+][A-])/[HA] pKa = -log Ka (proton donor) (proton acceptor) Conjugate acid-base pair Low Ka, high pKa High Ka, low pKa

  5. Formic acid has a pKa of 3.75; acetic acid has a pKa of 4.76. -Which is the stronger acid? -Does the stronger acid have a greater or lesser tendency to lose its proton than the weaker acid? -DRAW the titration curves of formic and acetic acids, on one graph. -At a solution pH of 4.76, what can you say about the concentrations of acetic acid (CH3COOH) and acetate (CH3COO-) present?

  6. Formic acid has a pKa of 3.75; acetic acid has a pKa of 4.76. -Which is the stronger acid? -Does the stronger acid have a greater or lesser tendency to lose its proton than the weaker acid? Formic acid is the stronger acid. It has a greater tendency to lose its proton than acetic acid; it "wants" to give away its proton. -DRAW the titration curves of formic and acetic acids, on one graph. (small group activity, with answers presented on the board) -At a solution pH of 4.76, what can you say about the concentrations of acetic acid (CH3COOH) and acetate (CH3COO-) present? At a solution pH of 4.76, the concentrations of acetic acid and acetate will be equal.

  7. Which of the following correctly describe(s) the parameter pKa? • the negative logarithm of the hydrogen ion concentration of an aqueous solution (2) a standard way to measure the [H+] concentration in an aqueous solution. (3) the negative logarithm of an equilibrium (or dissociation) constant (4) the pH at which a weak acid is one-half dissociated (5) the pH at which there are equal concentrations of a weak acid and its conjugate base (6) the pH at which maximum buffering capacity of the conjugate acid-base pair occurs

  8. Which of the following correctly describe(s) the parameter pKa? • the negative logarithm of the hydrogen ion concentration of an aqueous solution (2) a standard way to measure the [H+] concentration in an aqueous solution. (3) the negative logarithm of an equilibrium (or dissociation) constant* (4) the pH at which a weak acid is one-half dissociated* (5) the pH at which there are equal concentrations of a weak acid and its conjugate base* (6) the pH at which maximum buffering capacity of the conjugate acid-base pair occurs*

  9. Phosphoric acid, H3PO4 , is triprotic, with pKas of 2.14, 6.86, and 12.4. The ionic form that predominates at pH 3.2 is: A. H3PO4 B. H2PO4— C. H3PO3— D. HPO4 2— E. PO43—

  10. 1. Phosphoric acid, H3PO4 , is triprotic, with pKas of 2.14, 6.86, and 12.4. The ionic form that predominates at pH 3.2 is: A. H3PO4 B. H2PO4—* C. H3PO3— D. HPO4 2— E. PO43—.

  11. Catechols substituted with long chain alkyl groups are the components of poison ivy and poison oak that produce an annoying itchy rash (see structure below). If you were exposed to poison ivy while out walking in the woods, which of the treatments below would you apply to the affected area in order to make the below offending chemical the MOST soluble so it can be washed away? (pKa of the hydroxyl groups = 9)

  12. Wash the area with dilute vinegar or lemon juice (both acidic) • Wash the area with soap and water (soap is a Na+ or K+ salt of fatty acids) C. Wash the area with dilute vinegar or lemon juice and soap D. Wash the area with water and baking soda (alkaline) E. Wash with soap, water, and baking soda

  13. Wash the area with dilute vinegar or lemon juice (both acidic) • Wash the area with soap and water (soap is a Na+ or K+ salt of fatty acids) C. Wash the area with dilute vinegar or lemon juice and soap D. Wash the area with water and baking soda (alkaline) E. Wash with soap, water, and baking soda*

More Related