What is the pI value for aspartic acid, which has pKa values of 2.1, 3.9, and 9.8?
The answer is (2.1+3.9)/2 = 3.0
What happen to 9.8?? Why this number is not included?
What is the pI value for aspartic acid, which has pKa values of 2.1, 3.9, and...
A8 The acid dissociation constants (pKa) of the amino acid aspartic acid are shown below. What is the isoelectric point (pl) of this amino acid? pk, 9.8 ΤΗΝ PK, 2.1 TOH OS pk 3.9 ОН (A) 6.9 (B) 6.0 (C) 3.9 (D) 3.0 (E) 2.1
the two carboxylic acid groups of aspartic acid have different acidities with pKa values of 2.1 and 3.9. Predict which acid group is the more acidic by considering the effect of the -nh3+ group on the stability of the conjugate bases. Explain your reasoning.
Given the pKa values of Aspartate (2.1, 3.9 and 9.8), what is the net charge of Aspartate at: 1) pH = 13 (ANSWER SHOULD BE -2) Please show all calculations needed in order to get the answers in parentheses.
Aspartic acid has three pKa values, 2.09, 3.86 and 9.82. a. On the following structure for this amino acid circle the protons that can be removed and indicate the corresponding pKa value? b. Determine the value of the isoelectric point for this amino acid. c. Sketch the structure of the zwitterion. d. If electrophoresis is carried out at pH is 7.0, will this amino acid migrate to the anode(+) or cathode(-).
I dont really know how to do this question A8 Two acid dissociation constants (pka) of the amino acid aspartic acid are shown below. The measured isoelectric point (pl) is 3.0. What is the pka of the carboxylic acid side chain? PK, 9.8 pk, 2.1 *H3N он Questions continue over page
Consider a 0.203 L solution of the amino acid aspartic acid (0.615 M), which has an alpha carboxylic acid group (pka = 2.10), an alpha amine group (pka = 9.82), and a carboxylic acid group in the side chain (pka = 3.86). If the titration is started at a very low pH, how many liters of 2.15 M NaOH would you need to add to reach the isoelectric point of the amino acid? Give your answer to 3 significant figures...
H2A is a diprotic acid of which pKa values are 3.0 and 7.0. Answer to the following questions. (a) The pH of an aqueous solution prepared by dissolution of HzA can be approximately calculated by assuming that H2A is a monoprotic acid. Explain why this assumption is valid in terms of equilibrium constant and fractional composition. (10 pt)
(C) Water is less dense as a solid than as a liquid. (D) What has strong hydrogen bonding interaction between molecules, which allow it to have a high heat evaporation. (E) All of the listed properties of water make life possible. Aspartic acid is a weak amino, its structure is shown below. 10(60) 1) Draw a possible titration curve (pH versus [OH^-]) for 1 M aspartic solution. Indicate the pK_as in the graph (pK_1 = 2.1, pK_2 = 3.9 and...
help with this question Consider a 0.211 L solution of the amino acid aspartic acid (0.631 M), which has an alpha carboxylic acid group (pka = 2.10), an alpha amine group (pka = 9.82), and a carboxylic acid group in the side chain (pka = 3.86). If the titration is started at a very low pH, how many liters of 2.25 M NaOH would you need to add to reach the isoelectric point of the amino acid? Give your answer...
The amino acid glycine has pKa values of 2.4 and 9.8. A solution was made by dissolving 1.15 g of glycine sodium hydrate (shown below) in 100.00 mL of water. The molecular weight of the salt is 115 g/mol 5. Нас .Н20 Na+ H2N What is the pH of the salt solution? 20-mL aliquot of would result, making sure to label at least four sets of values on the graph. a ior itrated with 0.100 M b on curve that...