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 juiceC. 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

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 juiceC. 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

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)

WEAK acids and bases in biochemistry…

Tendency of an acid to dissociate HA<-> H+ + A- is described by

Ka = ([H+][A-])/[HA] pKpKaa = -log K = -log Kaa

(proton donor) (proton acceptor)

High Ka, low pKa

Low Ka, high pKa

Conjugate acid-base pair

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?    

 

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.  

Which of the following correctly describe(s) the parameter pKa?(1) 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

Which of the following correctly describe(s) the parameter pKa?(1) 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*

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. PO4 3—

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. PO4 3—.

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)

A. Wash the area with dilute vinegar or lemon juice (both acidic)

B. 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 

A. Wash the area with dilute vinegar or lemon juice (both acidic)

B. 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*