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Given,
pK1 = 7.57
pK2 = 9.30
pKD = 8.78
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- The ionization of p-nitrophenol is shown below (pKa = 7.0): a. Identify the weak acid and conjugate base. b. At pH 7, what are the relative concentrations of ionized and un-ionized p-nitrophenol? c. If enough concentrated hydrochloric acid is added to a solution of p-nitrophenol to lower the pH from 7 to 5, what will happen to the relative concentrations of the ionized and un-ionized forms? d. Ionized p-nitrophenol has a yellow color, while the un-ionized form is colorless. The yellow color can be measured using a spectrophotometer at 400nm. In order to determine the total amount of p-nitrophenol in a solution, would you perform the spectrophotometer reading at an acidic or basic pH? Clearly explain why? e. A solution of p-nitrophenol at pH 7.95 was found to have an A400 of 0.255 . What is the total concentration (in µM) of p-nitrophenol (ionized plus un-ionized) in the solution? The molar extinction coefficient of p-nitrophenol is 18,500 M-1cm-1 and the pKa is 7.Given the titration curve of the hypothetical polyprotic acid X at 0.100 M concentration (pKa1=4.0, pKa2=8.0, pKa3=12.0) titrated with 0.600 M NaOH, identify the pH at point C, H, E, and M.An enzyme (molecular weight= 24 kDa, pI= 5.5) is contaminated with two other proteins, one witha similar molecular mass and a pI of 7.0 while the other has a molecular mass of 100 kDa and a pIof 5.4. Suggest how the contaminated enzyme can be purified.
- You have an initial solution in which you added quantities of “A” and “B” such that there is 4.5 M “A” and 2.5 M “B” and no complex (“AB”) at time 0. After equilibrium, you are able to isolate and quantitate the “AB” complex, and find its concentration is 1.5 M. Given that RT is 0.59 kcal/mol, what is the delta Go’ for the association reaction?Each ionizable group of an amino acid can exist in one of two states, charged or neutral. The electric charge on the functional group is determined by the relationship between its pKa and the pH of the solution. This relationship is described by the Henderson-Hasselbalch equation.(a) Histidine has three ionizable functional groups. Write the equilibrium equations for its three ionizations and assign the proper pKafor each ionization. Draw the structure of histidine in each ionization state. What is the net charge on the histidine molecule in each ionization state?(b) Draw the structures of the predominant ionization state of histidine at pH 1, 4, 8, and 12. Note that the ionization state can be approximated by treating each ionizable group independently.(c) What is the net charge of histidine at pH 1, 4, 8, and 12? For each pH, will histidine migrate toward the anode (+) or cathode (−) when placed in an electric field?In proteins involved in blood clotting to heal a wound, the amino acid GLU is often chemically modified to carboxy-glutamic acid (abbreviated GLA, shown in diagram at pH 7) by a carboxylase enzyme in the blood. The pKa values for the two ionizable protons in the R-group of GLA are shown. A sample of the octopeptide ILE-GLA-ARG-GLY-MET-ARG-PHE-SER was digested with trypsin, adjusted to pH 13, and applied to an anion exchange column. The peptides were then eluted from the column using a pH gradient from 13 to 0.5. Write the order of the products (no structures required) at the pH they would elute from the column and indicate the pH value. Assume pKa values for any newly generated a-amino and a-carboxyl groups are 9.6 and 2.2 respectively. (Relevant pKa values are 2.2, 3.2, 4.8, 9.6, and 12.5).
- The activity of an enzyme requires a glutamic acid to display its -COOHfunctional group in the protonated state. Suppose the pKa of the -COOHgroup is 4.07.(a) Will the enzyme be more active at pH 3.5 or 4.5? Explain.(b) What fraction of the enzymes will be active at pH = 4.07? Explain.(c) At what pH will the enzyme show 78% of maximal activity?Given a tripeptide Cys-His-Lys, Cys: Pk1 = 1.71; Pk2 = 10.78; PkR = 8.33 His: Pk1 = 1.82; Pk2 = 9.17; PkR = 6.0 Lys: Pk1 = 2.18; Pk2 = 8.95; PkR = 10.53 draw the protonic equilibria for the tripeptide what is the IpH? What is the dominant structure at pH 2.0? What is the first buffering region of the tripeptide?Each ionizable group of an amino acid can exist in one of two states, charged or neutral. The electric charge on the functional group is determined by the relationship between its pKa and the pH of the solution. This relationship is described by the Henderson-Hasselbalch equation. Lysine has three ionizable functional groups. The pKa for these groups are pK1 = 3.1, pK2 = 8.3 and pKR = 10.8. 1. Draw the structures of the predominant ionization state of Lysine at pH 1, 4, 8, and 12. Calculate also the net charge of each of these ionized molecules. Show your work. 2. Calculate the isoelectric point (pI) of Lysine in aqueous solution using the pKa values given above. Explain the rationale of your calculations and show your work.
- Histidine is frequently used as a general acid or base in enzyme catalysis. Considering the pKa value of the side chain, suggest a reason why is this so?Using Figure 1.3 of the Introduction as an example, a) draw all the structures of the tribasic amino acid lysine involved in the equilibrium reactions that would take place during titration against NaOH, starting with the fully protonated form below (draw the R-group in full). HAN+-CH- COOH (CH2)4 NH°+ b) indicate the numerical pa value of each equilibrium reaction, and which ionizable group is being dissociated in each step. c) indicate the net charge of the amino acid at each step and identify the zwitterion. d) Calculate the pI of this amino acid (show the calculation). e) What would be the predominant ionization states of this amino acid at physiological pH (7.4) and at this pH, what would the ratio of these two states be (show the calculation)?1.2. Using DEAE-cellulose as ion exchange resin, indicate the starting and ending pH for the narrowest experimental pH range used to separate an amino acid mixture consisting of Cys, His and Leu Starting pH: _____ Ending pH: _____