Determine the net charge of the predominant form of Asp at (a) pH 1.0, (b) pH 3.0, (c) pH 6.0, and (d) pH 11.0.
1 answer:
Answer:
a) +1
b) 0
c) -1
d) -2
Explanation:
The aspartic acid is one of the twenty amino acids that make up proteins.
The equilibrium is in the image. pka for this molecule are 1.88, 3.65 and 9.60. A higher pH than pka will have as predominant form the molecule in the right and vice versa. The net charge in each molecule is in red.
Thus, for a pH of 1.0, as the pH is lower than first pka, predominant form will have a net charge of +1. If pH is 3.0, predominant form will have a net charge of 0. If pH is 6.0 predominant form will be the -1 and for a pH of 11.0, predominant form is the -2.
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Answer:
See the explanation
Explanation:
In this case, in order to get an <u>elimination reaction</u> we need to have a <u>strong base</u>. In this case, the base is the phenoxide ion produced the phenol (see figure 1).
Due to the resonance, we will have a more stable anion therefore we will have a less strong base because the negative charge is moving around the molecule (see figure 2).
Finally, the phenoxide will attack the <u>primary carbon</u> attached to the Cl. The C-Cl bond would be broken and the C-O would be produced <u>at the same time</u> to get a substitution (see figure 1).
