Calculate the volume, in liters, of 1.690 M KOH that must be added to a 0.112 L solution containing 9.27 g of glutamic acid hydrochloride (H3Glu*Cr, MW = 183.59 g/mol) to achieve a pH of 10.16. Glutamic acid (Glu) is an amino acid with pK, values of pka1 = 2.23, pK2=4.42, pka3 =9.95. Number 0.136479 L NH₂* CI™ CH-CH₂-CH2₂ مال -OH OH Glutamic Acid Hydrochloride

Calculate the volume, in liters, of 1.690 M KOH that must be added to a 0.112 L solution containing 9.27 g of glutamic acid hydrochloride (H3GluCr, MW = 183.59 g/mol) to achieve a pH of 10.16. Glutamic acid (Glu) is an amino acid with pK, values of pka1 = 2.23, pK2=4.42, pka3 =9.95. Number 0.136479 L NH₂ CI™ CH-CH₂-CH2₂ مال -OH OH Glutamic Acid Hydrochloride

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...

See similar textbooks

Similar questions

You dissolve 5.3 g of ascorbic acid (MW 176; pk 4.2, 11.6) in 150 mL of water. When the solution comes to equilibrium, what is the pH?
Kk.268.
Consider acetic acid. What is the net charge on the molecule in a solution of acetic acid at pH of 5.8, 4.8, 8.4 and 1.5. The pKa of acetic acid is 4.8.
Based on the graph below, 1. molar concentration of HCO3- 2. alkalinity in ppm CaCO3
Phenolphthalein has a pKa of 9.7 and is colorless in its acid form and pink in its basic form. For pH= 7.7 calculate [In−]/[HIn]. Express your answer using two significant figures.
Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant. What substance served as the primary standard?Which served as the indicator in the titration?What is the color at the end point?What is the concentration of the titrant?What is the molar concentration of the acetic acid solution?
A student added a total of 75 mL sodium hydroxide to titrate an amino acid solution with 0.5M NaOH. They also calculated that they added a total of 14 mL of sodium hydroxide to arrive at pH 2.6 and a total of 32 mL of sodium hydroxide to arrvive at pH 4.8.What was the initial concentration of the amino acid solution in milimolar (mM)? The calculations must be presented such that those can be recapitulated by the marker. Provide the answer with no decimal places. Show all details of your working out. State the answer in a full sentence.
Given an amino acid, be able to draw the structure when it is placed in water at pH = 2, pH = 7, or pH = 13. Is the amine group protonated or not? Is the carboxylic group protonated or not?
Q2
What would the [H3O*] be if you had a solution of 0.125 M solution of the zwitterionic form of Tyrosine? (pKa1 = 2.20; pka2 = 9.11) 1.26 x 10-2 M 2.16 x 10-6 M 2.51 x 10-2 M 7.88 x 10-5 M
The pka's of the ascorbic acid are pka1 = 4.10 and pka2 = 11.80. If the net charge of ascorbic acid is exactly -1, what is the pH of the solution? Use 2 decimal places.
Calculate the pH of a 0.50 M tartaric acid solution (pK₁1 = 2.89; pK₁2 = 4.40). Express your answer using two decimal places. 15| ΑΣΦ ?