Calculate the pH, [H2L*], [HL], [L] for each solution of the amino acid proline (Kal = 1.12 x 102 (COH) and K2 = 2.29 x 101 (NH3)) when the solution is a. 0.0243 M H2L* b. 0.0732 M L c. 0.0449 M HL %3D
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![Calculate the pH, [H2L*], [HL], [L] for each solution of the amino acid
proline
(Kai = 1.12 x 102 (COH) and K2 = 2.29 x 1011 (NH3)) when the solution is
a. 0.0243 M H2L*
b. 0.0732 M L
c. 0.0449 M HL](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F141c66cb-062d-4578-8c17-7fdb89d3aa91%2F3aeb521f-c9ae-4a31-af87-5df8957376b2%2F5nxcgx6_processed.jpeg&w=3840&q=75)
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- You are given 0.5 M solution of the amino acid Arginine. pK1 (α-carboxyl group) = 2.17 pK2 (α- amino group) = 9.03 and pK3 (guanidine group) = 12.48 Answer the following questions. a. Determine the pH of the solution if you add 15 mL 0.25 M HCl to 10 mL of the 0.5 M Arginine. Assume that Arginine is in isotonic state. Show all calculations. Draw the structure of the amino acid at the pH determined in question 1a.n the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of diethylamine, (C2H5)2NH to be 12.177. Use the information she obtained to determine the Kb for this base. Kb(experiment) =All amino acids have two ionizable functional groups: an α‑amino group (average p?a of 9.4) and an α‑carboxylic acid group (average p?a of 2.2). Aspartic acid has an ionizable side chain (R group) with a p?a of about 3.8. One of the possible ionization states of aspartic acid is shown in the image. The protonated form of the R group of aspartic acid is shown in the structure. The ratio of the protonated form to the charged (deprotonated) form depends on the p?a of the R group and the pH of the solution. Select all the pH values at which the charged form of the R group would predominate.
- 1) You are asked to prepare a buffer for a protein assay. This protein works best at a slightly acidic pH of 5.5. a. From the list of Acids and conjugate bases which pair would you pick. (The list is in the attached image) b. You are asked to make a 1M stock solu on of the Buffer, how many grams of each acid and base would you need to make a 500mL stock. c. For the experiment, the final concentra on of the buffer should be 50mM. How many mL of your stock would you need to make 2L. Hint: M1V1=M2V2Calculate the pH of a .5M solution of the amino acid, aspargine, that was prepared from the form of asparganine that has a net -1 charge. Ka(-COOH) = 6.92x10^-3 and Ka(-NH3+)=1.86x10^-9 A. 4.52 B. 1.23 C. 5.45 D. 11.22 E. 7.93 F. 10.42Find the pH of a solution 2.0 M in ethylamine CH3CH2NH2. For CH3CH2NH2 Kb=5.6x10-4. Explain step by step as you set up the equation and what each element represents.
- How to answer for Ka/ Kb and calculated pH of a solution? I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Ex. Solution 1: 30.0 mL 0.10 M CH3COOHSolution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COOSolution 3: 30.0 mL 0.10 M NH3Solution 4: 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl Sol 1,2 used methyl orange as indicatorSol 3,4 used phenolphthalein as indicator Solution w/ measured pH Ka/Kb Calculated pH 1 a 1.0 M HCl (2.01pH) b 1.0 M NaOH (3.98pH) c Control (2.91pH) 2 a 1.0 M HCl (4.73) b 1.0 M NaOH (4.82) c Control (4.76) 3. a 1.0 M HCl (10.09) b 1.0 M NaOH (11.98) c Control (11.11) 4. a 1.0 M HCl (9.13) b 1.0 M NaOH (9.38) c Control (9.30)You are preparing a sample for Kjeldahl analysis. Based on the protein information in the sample, you need to use a buffer with pH=8. Which of the following weak base and its conjugate acid will you use? a. NH2OH, pKb = 8.04b. CH3CH2NH2, pKb = 3.37c. NaH2PO4, pKa = 7.21For a weak acid with a pKa of 6.0, show how you would calculate the ration of acid to salt at pH 5.
- Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His = imidazole group). A biochemist makes up 100 mL of a 0.100 M solution of histidine at a pH of 5.40. She then adds 40 mL of 0.10 M HCl. What is the pH of the resulting solution?Calculate the pH of 50mls of 0.1100M arginine to which 20 mls PH of 0.1005M Hcl have been added.Give typed full explanation not a single word hand written otherwise leave it Calculate the isoelectric point of the amino acid histidine by plotting the titration curve. (pka values α-COOH=1.82, α-NH2= 9.17, imidazole= 6.0)