Fig. 1 shows the possible effect of pH on recovery and impurity removal at the selection of a setpoint that allows for process control and enables a robust method. At what pH the recovery is at its highest and the impurities near their lowest. Also explains the intersection of two lines at pH 5.5. PROTEIN PURIFICATION METHODS 90 80 70 60 - Recovery (%) 50 -Impurity Concentration (ng/ml) 40 30 20 10 4.5 5.0 5.5 6.0 6.5 7.0 7.5 8.0 8.5 pH Recovery (%) or [Impurity] (ng/mL)

Fig. 1 shows the possible effect of pH on recovery and impurity removal at the selection of a setpoint that allows for process control and enables a robust method. At what pH the recovery is at its highest and the impurities near their lowest. Also explains the intersection of two lines at pH 5.5. PROTEIN PURIFICATION METHODS 90 80 70 60 - Recovery (%) 50 -Impurity Concentration (ng/ml) 40 30 20 10 4.5 5.0 5.5 6.0 6.5 7.0 7.5 8.0 8.5 pH Recovery (%) or [Impurity] (ng/mL)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

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665 mL of 0.875 M aqueous aniline solution CC 2H5 NH2) are boiled gently to reduce the volume to 401 m L. The solution was then left to disociate , and the Kb of this Solution was found to be 3.9X10-10.Estimate the pi of aniline at eguilibrium Identify the conjugated acid-base pair according to Bronste d - Lowry Theory of the dissoci ati on reaction of aniline (CH5 NH2). Calculate the ka value Of the reaction
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a) Over 80 % industry area has reported acid rain due to harmful gases emissions. Josephine collected a rainwater sample from industry site and analysed it using pH meter. It was found that the sample recorded an average pH of 4.35. Calculate the amount of H* in rainwater sample. Suggest an alternative method to determine H* in unknown liquid samples.
FREE RESPONSE 12 J1.30 10 9,60 (IV) 8. pH 6 5.97 CIII) 4 2.34 (1I) (I) 0.5 1.0 1.5 2.0 OH- (equivalents) 1. In your laboratory exercise you titrated 100 mL of solution of 0,1 M glycine at pH 1.72 with 2M NaOH solution. She monitored the pH and plotted the graph shown above. For each of the following statements, identify the appropriate pH in the titration. (a) The pH at which average net glycine is +0.5. (b) The pH that is equal to the pKa of the protonated amino group. (c) The pH at which the predominant glycine species is "NH3-CH2-COOH (d) The pH at which the average net charge of glycine is -1 (e) The isoelectric pH (pl) of glycine. 2.
Analysis of an amine using a back-titration Kjeldahl method resulted in the following equation for P, the percent nitrogen in the amine: P = (mmols acid) – (mL base) (molarity base) (14.01) (100) (mg sample) = (4.75 ± 0.03 )- (0.1198) ± 0.0008) (15.00 ± 0.04) (14.01 ) (100) 750.0 ± 0.3 where the uncertainties are all standard deviations for infinite -sized samples. How will you report the value for P?
The pK, values for the amino acid leucine (R = CH2CH(CH3)2) are pKa1 = 2.36 and pKa2 = 9.60. Fill in the correct value or word to complete each sentence below. At what pH value will the isoelectric point, pl, occur? The pl will occur at pH = At pH = 2.00, the predominant species of leucine in solution has an overall charge.
In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of trlethylamine, (C₂H5)3N to be 12.202. Use the information she obtained to determine the K, for this base. K(experiment) = Submit Answer $ 4 000 000 R F F4 V % 5 T G Retry Entire Group 9 more group attempts remaining FS Cengage Learning | Cengage Technical Support B ^ 6 MacBook Air Y F6 H & 7 ◄◄ U F7 J * 00 8 N M F8 I K ( 9 ►► + = { 1 11 Save and Exit F12 B 1 delete
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www-awu.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNsIRI 18.3 Gibbs Free E... 5.3 Enthalpies of.... ! Q = @ 2 O ACIDS AND BASES Preparing a strong base solution with a given pH W A chemist must prepare 650.0 mL of sodium hydroxide solution with a pH of 13.70 at 25 °C. She will do this in three steps: • Fill a 650.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. . Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. S Explanation #3 3 JUF 18.5 Gibbs Free E... Check E $ 4 R X % 5 S Reading Schedule 19.6 Reduction Po... Y SOLUTION: The le... I stv T M MacBook Pro A 6 Y Is & 7 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Pri τα 7 U * The 8 O 9
Water sample from different river water was subjected to a qualitative alkaline analysis by titrating against 0.1250 MHC1 and using phenolphthalein and bromocresol green end point. The table below shows the volumes of acid needed to titrate 25.00-mL portions of each sample and their corresponding end point, separately. Use this information to deduce the composition of the solutions. Calculate the molar concentration of each solute. Volume (mL) Phenolphthalein end Bromocresol green Solute identity concentration end point Volume (mL) Molar Sample point 22.40 of solute/s 1 22.41 2 0.00 33.40 3 15.67 42.13 4 29.64 36.42