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Chapter 2: Q9. (page 40)
Draw the structures of the conjugate bases of the following acids:
(a) (b)
The structure of the conjugate bases are shown below.
(a) (b)
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Use Coulomb鈥檚 law (Equation 2-1) to explain why a salt crystal such as NaCl remains intact in benzene (C6H6) but dissociates into ions in water.
Calculate the of a solution containing
(a) of ,
(b) of glycine and of , and
(c) of acetic acid and of sodium acetate (formula weight ).
You need a buffer at for use in purifying a protein at . You have chosen Tris, . You carefully make up Tris buffer, at data-custom-editor="chemistry" , and store it in the cold to equilibrate it to the temperature of the purification. When you measure the of the temperature-equilibrated buffer it has increased to . What is the explanation for this increase? How can you avoid this problem?
Why is it important to maintain biological molecules in a buffered solution?
Glycine hydrochloride is a diprotic acid that contains a carboxylic acid group and an ammonium group and is therefore called an amino acid. It is often used in biochemical buffers.
(a) Which proton would you expect to dissociate at a lower pH, the proton of the carboxylic acid group or the ammonium group?
(b) Write the chemical equations describing the dissociation of the first and second protons of .
(c) A solution containing and of the monodissociated species has . What is the of this dissociation?
(d) In analogy with Figure , sketch the titration curve of this diprotic acid.
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