The relative polarities of a few common solvents are given below: Solvent name Relative polarity Water 1 Acetic acid 0.65 Acetonitrile 0.48 While using a C-18 hydrocarbon column for protein purification, which of the following will be the best elution solvent mixture? The final polarity of the solvent mixture can be predicted by considering the relative % of each constituent and their respective relative polarity values provide. 1. 90% water and 10% acetic acid II. 90% acetic acid and 10% acetonitrile III. 90% acetonitrile and 10% water IV. 10% acetonitrile and 90% acetic acid

The relative polarities of a few common solvents are given below: Solvent name Relative polarity Water 1 Acetic acid 0.65 Acetonitrile 0.48 While using a C-18 hydrocarbon column for protein purification, which of the following will be the best elution solvent mixture? The final polarity of the solvent mixture can be predicted by considering the relative % of each constituent and their respective relative polarity values provide. 1. 90% water and 10% acetic acid II. 90% acetic acid and 10% acetonitrile III. 90% acetonitrile and 10% water IV. 10% acetonitrile and 90% acetic acid

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

Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin itcauses the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of methemoglobin whichcannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base.C6H5NH2 (aq) + H2O (ℓ) ⇋ C6H5NH3+ (aq) + OH- (aq)a. When you measure the concentrations of the ionized substances you find them to be:[C6H5NH2] = 0.234 mol/L [C6H5NH3+] = 2.8 x 10-5 mol/L [OH-]= 2.8 x 10-5 mol/LIf the Kb is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (rightor left) to reach equilibrium? Explain. b. At equilibrium the concentrations of the ionized substances are:[C6H5NH2] = 0.0537 mol/L [C6H5NH3+] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 mol/LIf this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to thereaction, what will the new concentrations of the three ionic species be when…
There are two pH values in which Glutamic acid will have an a complete net charge of 2.17? what is the lowest PH1 and highest of pH2 round your amswers to the nearest 0.1 no orher information was provided
Calculate the pH at 25 °C of a 0.32M solution of trimethylammonium chloride ((CH3)2NHCI). Note that trimethylamine ((CH3)3N) is N is a weak base with a pK of 4.19. Round your answer to 1 decimal place. = 0 pH =
mm 0.022 doidve of (41) bros Sibisconbydlo noitudo: M ILL 6. Classify each of the following as an Arrhenius acid (AA), a Arrhenius base (AB), a Bronsted-Lowry acid (BLA), a Bronsted-Lowry base (BLB), a Lewis acid (LA), and/or a Lewis base (LB). Select all that apply. Cact to nous dinoj Jusoraq silt ei ted You may need to draw the Lewis structure of some molecules to make this determination. The pKa of hydronium ion is -1.7. a. H₂O BLA LA BLB LB b. HI (pKa = -8) AA AB BLA BLB LA LB c. BH3 (pKa = ∞ BLA BLB LA LB d. NaOH AA AB BLA BLB LA LB e. CH3CH₂OH (pka = 16) AA BLA LA f. NC13 AA BLA LA AB BLB LB AB BLB LB g. NH3 (pKa = 39) AA AB BLA BLB LA LB h. F- AA BLA LA AB BLB LB
In the gas phase the base strength of amines increases along theseries:NH3 < CH3NH2 < (CH3)2NH < (CH3)3NDiscuss the effects determining this order
For a 0.315 M solution of H₂C6H606, calculate both the pH and the C6H₂06²- ion concentration. = 7.9x10-5 H₂C6H6O6 + H₂O — H3O+ + HC₂H0¯ Ka¹ HCH6O6 + H2O=H3O+ + CoH6O2- Ka2 = 1.6×10-12 pH = [C6H606²-] = M
A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500. mL of solution. What is the bromide ion concentration in this solution? 20 Multiple Cholce X 0206:02 9.19 x 10-3 M 230 x 10-2 M 272 x 10-3 M 1.84 x 10-2 M 1.25 x 10-1 M Mc Graw Hill Type here to search 近 C
Calculate the pH at 25 °C of a 0.18M solution of lidocaine HCI (C14H21 NONH₂C1). Note that lidocaine (C₁4H21NONH) is a weak base with a pK, of 7.94. Round your answer to 1 decimal place. pH = 1 X
For a 0.143 M solution of H2C6H6O6, calculate both the pH and the C6H6O62- ion concentration. H2C6H6O6 + H2O H3O+ + HC6H6O6- Ka1 = 7.9×10-5 HC6H6O6- + H2O H3O+ + C6H6O62- Ka2 = 1.6×10-12 pH = [C6H6O62-] = M
Calculate the pH at 25°C of a 0.64M solution of anilinium chloride C6H5NH3Cl. Note that aniline C6H5NH2 is a weak base with a pKb of 4.87.
The amino acid L-histidine (L-His) has a side chain with a functional group called an imidazole, which in its protonated form has a pK₂ of 6.9. Draw its four different ionization states in water at the pH values indicated. Write the total charge on the molecule in the box at the bottom. pH = 8 is done for you. pH = 0 pH = 4 pH = 8 pH =12 +H3N. 요. N= 0 ΝΗ
The following compounds are available as 0.10 M aqueous solutions: pyridine triethylamine m-nitroaniline NaOH phenol HCIO HCIO4 (рКь = 8.82) (pKb = 3.25) (pKb = 11.53) (K₂ = 1.1 × 10-10) (K₂ = 2.9 × 10-8) Which two solutions could be combined to prepare a pH 6.7 buffer? HCIO and NaOH phenol and NaOH m-nitroaniline and HCIO4 pyridine and HCIO4