(a) Illustrate a titration curve of the following structure. (Solid lines indicate covalent bonds)Indicate buffering regions (including size) and the isoelectric point, pl.Asn - Cys - AlaLys-Cys -Phe(b) What is the predominant charge state at the following pH values? pH 1, pH 4, pH 7, pH 11(c) What would you expect to happen to your titration curve if you exposed this peptide to Beta-mercaptoethanol prior to titration? Describe the changes in the titration curve.(d) If this compound was subjected to an amidation at the Carboxy-terminus of Alanine, how doyou think the charge state would change?

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Determine the pH of a 10-3 mol/L solution of (a) hydrogen sulfate ion (pKa = 1.99), (b) formic acid (pKa = 3.75), (c) hypochlorous acid (pKa = 7.53), (d) phenol (pKa = 9.98)
Consider the titration of 40,0 mL of 0.0600 M H₂NNH₂ (a weak base; K = 1.30e-06) with 0.100 M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (d) 18.0 ml pH = (b) 6.0 mL pH = (e) 24.0 mL pH = (c) 12.0 mL pH (f) 36.0 ml. pH = 4
4. In the titration of15.00 mL of 0.200 M HC with 0.100 M NaOH, calculate the pH after the addition of the following volumes of titrant (mL) ; (a) 0.00; (b) 10.00; (c)14.50 ; (d) 15.00; (e) 15.50: (f) 20.00 mL.
Determine the pH of the buffer solution prepared by adding 40.0 mL 0.200 M H3PO4 and 50.0 mL 0.300 M NaOH in a 500 mL beaker. (pKa,1 = 2.10, pKa,2 = 7.20, pKa,3 = 12.0) The answer for this problem is given as 8.05, but I am having difficulty with the process on calculating that. Please show the step-by-step computation for this. Thank you!
14- Triethylammonium chloride (22.00g, (C2H5);NHCI, 137.65 g/mol) is added to water to make 1.75 L of solution. (Hint: (C2H5);NH* is the conjugate acid of the weak base triethylamine, (C2H5);N, pKs = 4.19). A buffer is prepared by mixing 25.00 mL of the previous solution with 25.00 mL of 0.0750 M sodium hydroxide. Determine the pH of the resulting buffer. 15- A buffer is prepared using 0.180 mol of dihydrogenphosphate ions and 0.120 mol of hydrogenphosphate ions in 250.0 mL volumetric flask. a- Calculate the pH of the prepared buffer.
Calculate the pH at the equivalence point in titrating 0.066 M solutions of each of the following with 0.061 M NAOH. (a) periodic acid (HIO4) pH = (b) benzoic acid (HC;H502), K, 6.3e-05 pH = (c) acetic acid (HC2H302), K - 1.8e-05 pH -
A biochemist prepares two stocks of sodium phosphate buffer by titrating phosphoric acid with sodium hydroxide. She prepares a 0.10 M solution of sodium phosphate buffer at pH 2.15, and she prepares a 0.10 M solution of sodium phosphate buffer at pH 7.20. If she mixes 48 mL of the pH 2.15 buffer with 29 mL of the pH 7.20 buffer, what will be the pH of the resulting solution? Recall that the pKas of phosphoric acid are 2.15, 7.20, and 12.35. Enter your answer to the nearest hundredth.
I dont know how to do this question.
Consider the titration of 25.00mL of 0.200M methylamine (CH3NH2). The titrant is 0.120M HCl. (Calculate each below using ICE and ICF tables.) Note you should NOT use M1V1=M2V2 (a) the initial pH of base? (b) the pH at 5.00mL added? (c) the pH at 1/2 the HCl needed to reach the equivalence point. (d) the volume of added acid required to reach the equivalence point? (e) the pH at equivalence point.
Use Figure to find an indicator for these titrations:(a) 0.10 M CH₃NH₂ with 0.10 M HCl(b) 0.50 M HI with 0.10 M KOH
Read sec. 14.7 2, then calculate the volume at equivalence and the pH at each of the following volumes of titrant for the titration of a 75.00 mL of a 0.049 mol L1 solution of nitrous acid (pKa = 3.37) titrated with 0.198 mol L' sodium hydroxide. %3D Ve = 18.6 mL VOH pH VOH 7.05 pH : VOH = = 12.1 pH %3D VOH = Ve %3D pH %3D Von = 27.8 pH = VoH = 55.7 pH Submit Question Jump to Answer
2. Joey was tasked to ensure that an enzyme responsible for keeping his species from extinction remains biologically active. To do so, he needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt KYA Benzoic acid, C6H5COOH 6.25 x 105 NaCH₂COO MUH Boric acid, H3BO3 5.81 x 107 NaH₂BO TWO Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (KYA, MUH, or TWO) will Joey store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 1.75 M stock solution (pH 7.00) of the same buffer system needed to prepare 250 mL of a 0.550 M buffer pH 7.00. After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as…

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