Can you help me to explain to me? 13.4) In the previous problem, you drew the predominant form of leucine at pH = 1.0, pH = 7.4, and pH = 12.0. These structuresare shown below. What is the total charge of leucine at pH = 1.0, pH = 7.4, and pH = 12.0?HH-NHpH = 1.0H :0:I ||сCH₂|CHCH3-Ö-HCH3total charge = 1+There is a formal charge of 1+ on thenitrogen.physiological pH (pH = 7.4)HH :0:1||-C-0:H-|HCH₂|CHCH3|CH3total charge = 0There is a formal charge of 1+ on thenitrogen, and a formal charge of 1- onthe oxygen. Adding these charges givea total charge = 0.pH = 12.0H|H-N-:0:||HCH₂|CHCH3TCH3total charge = 1-There is a formal charge of 1- on theoxygen.

Amino acids are biomolecules that have an amino group and a carboxyl group linked to the same carbon…

Answered: 13.4) In the previous problem, you drew…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Draw dipeptide Arg-Thr at pH 6.0. Circle the six atoms that are restricted in one plane. Calculate its approximate pI assuming pKa for NH3+ is 10.0, pKa for COOH is 3.0, PKR for Arg is 12.0
The amino acid glycine is often used as an ingredient in buffers for biochemistry experiments. The amino group of glycine has a pKa of 9.6. Glycine exists in either a protonated form (-NH3+) or a free base (-NH₂). a) In what pH range can glycine be used as an effective buffer? b) In a 0.1M solution of glycine at pH 9.0, what fraction has its amino group in the protonated form? c) When 99% of the glycine is in the protonated from, what is the numerical relation between the pH of the solution and the pKa of the amino group?
The structure of chitosan, a polymer used to eliminate protein clumps that create wine haze in white wine, is shown below. The amine functional group on chitosan has a pka of 6.5 in its conjugate acid form. What is the charge state of the amine group of chitosan in wine with a pH of 3.6, given the following acid-base reaction, where chitosan is abbreviated as R? (If you need it, the Henderson-Hasselbach connection is also provided.) [RNH2] [RNH;] NH2 RNH2 + H20 2 RNH + 0H- pH = pKa+ log OH n a) At pH 3.6, it is negatively charged; b) At pH 3.6, it is positively charged; c) At pH 3.6, it is both positively and negatively charged; d) At pH 3.6, it is neutral.
Based on the following titration table of Glycine, would you be able to recreate the same for Histidine? Glicina Increasing pH H-N-CH,-COOH -H-N-CH,-co = H-N-CH,-C00- Net charge: +1 pH COOH-pKa = 2.3 NH3-pka = 9.6 CN AEq +1 +1 2.3 (0.5°-1)+(0.5°0)=-0.5 +0.5 0.5 9.6 -1 (0.5*+1)+(0.5°0)=+0.5 -0.5 1.5 14 Given that the pKas for Histidine are the following: pka1 = 1.82 pKa2 = 9.17 pКаз %3 6.00 pL = 7.59 2.
At a pH equal to the isoelectric point of alanine, the net charge on alanine is zero. Two structures can be drawn that have a net charge of zero, but the predominant form of alanine at its pI is zwitterionic.(a) Why is alanine predominantly zwitterionic rather than completely uncharged at its pI?(b) What fraction of alanine is in the completely uncharged form at its pI? Justify your assumptions.
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.
Identify the acid on the left and its conjugate base on the right in the following equations:(a) HOCl + H2O ↔ H3O+ + OCl-(b) HONH2 + H2O ↔ HONH3+ + OH-(c) NH4+ + H2O ↔ NH3 + H3O+(d) 2HCO3-2 ↔ H2CO3 + CO3-2 (e) PO4-3 + H2PO4- ↔ 2HPO4-2
One liter of a 0.1 M Tris buffer (pKa of Tris = 8.3, see Table 2.4) is prepared and adjusted to a pH of 2.0. A) What are the concentrations of the conjugate base and weak acid at this pH?Answer with 2 significant digits. I have solved for [HA] = 0.10 Can you please help solve for [A-] = ?
A sample (660 mg) of a (homo)oligomeric protein of molecular weight of 132,000 Da was treated with an excess of 2,4-dinitro-fluorobenzene until the reaction was complete. The peptide bonds were then completely hydrolyzed by heating with 6 M hydrochloric acid. The hydrolysate was found to contain 5.5 mg of the following compound. NO2 O2N- NH НООС 2,4-Dinitrophenyl derivatives of the amino groups of other amino acids were not found. a). How many polypeptide chains are there in this protein? Show your work. b). Assuming that each of the subunit contains entirely a-helices, how many a-helical turns would there be, approximately, in each of the subunit? "For a protein of typical composition, average amino acid residue mass is ca. 110 Da."
b) Determine which ionization state corresponds to aspartic acid (shown below) at pH 1, 7, and 10 by selecting the most suitable answer from the statements i-iv. The pK of the amine, carboxylic acid, and side chain of aspartic acid are 9.6, 1.88 and 3.65, respectively. ОН ÓH ÑH2 i) the amine is charged; the carboxylic acids are neutral. ii) the amine and carboxylic acids are all charged. iii) the amine is neutral, and the carboxylic acids are charged. iv) the amine and the carboxylic acids are all neutral. pH Statement (i, ii, iii, or iv) 1 7 10 %3D
The following amino acid is dissolved in solution at pH 7.4. HC H' + CH CH₂ H/ H+ HC a. Which amino acid is this? (all lower case) N- H CH CH₂ b. What is the pKa of its ionizable side chain? (Use the value from the textbook.) c. What is the ratio of the uncharged to the charged form at pH 7.4? (write answer as number with one decimal place, ex 2.5 or 0.2 or 50.0 with an implicit "to 1")
The PI of protein P is 7.3. One can purify protein P by: Anion-exchange chromatography at pH 2.0 Anion-exchange chromatography at pH 7.3 Anion-exchange chromatography at pH 9.0 Anion-exchange chromatography at pH 4.3

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