If this biomolecule was placed into a buffer at a pH of 5.0 in a charged environment would it movetowards the postive or negative terminal?H3N-CH- CNH–CHC-NH–CHOHCH2CH3CH2CH2C-OHOit is neutral so would not move○ positive○ negativeICH2CH2NH3

If the biomolecule is placed into a buffer at a pH of 5.0 in a charged environment, its movement…

Answered: If this biomolecule was placed into a…

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 125CP: Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to...

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Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Write the values of Y and X. H2SO4 CH3CH=CH2 + H2O CH;CH-CH2 H HỌ 2-propanol an alcohol The pKa of a protonated alcohol is about -2.5, and the pKa of an alcohol is about 15. Therefore, as long as the pH of the solution is greater than Y and less than X, more than 50% of 2-propanol will be in its neutral, nonprotonated form. Express your answers using two significant figures separated by a comma. AX中 Y, X = %3|
20. Which of the following acid/ conjugate base pairs would function best as a buffer at physiological pH? a Lactic acid / Lactate ion; pKa = 3.86 b Carbonic acid / Bicarbonate ion; pKa = 6.37 c Bicarbonate ion / Carbonate ion; pKa = 10.25 d Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86 e Acetic acid / Acetate ion; pKa = 4.76
Consider a buffered solution containing CH³NH3Cl and CH3NH₂. Which of the following statements concerning this solution are TRUE? (Ka (CH3NH3†) = 2.0 × 10-¹¹) (A) A solution consisting of 0.10 M CH3NH3Cl and 0.10 M CH3NH₂ would have a higher buffering capacity than one containing 1.0 M CH3NH3Cl and 1.0 M CH3NH₂. (B) If [CH3NH₂] > [CH3NH3*], then the pH is larger than the pKa value of CH3NH3*. (C) Adding more [CH3NH3Cl] to the initial buffer solution will increase the pH. (D) If [CH3NH₂] > [CH3NH3*], then pH > 10.50. (E) If [CH3NH₂] = [CH3NH3*], then pH = 3.30.
You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC2H3O2] + [C2H;O2] = 0.250 M) at pH 3.50. How many mL of 1.000 M NaOH must you add in order to change the pH to 5.37? Acetic acid has a pka of 4.74. mL 1 2 3 4 C 7 8 9. +/- х 100 +
Q7. Given the following Ka values for the weak acids and bases: CH;COOH/CH3CO0 HCO3/CO32- H2PO4 /HPO,2 Ка 1.8 х 105 Ka = 5.6 x 10:11 Ka = 6.2 x 108 Which of the pair(s) would be appropriate as a buffer at pH = 7.0? Explain your answer.
Which of the following acid/ conjugate base pairs would function best as a buffer at physiological pH? Lactic acid / Lactate ion; pka = 3.86 Carbonic acid / Bicarbonate ion; pka = 6.37 Bicarbonate ion / Carbonate ion; pKa = 10.25 Dihydrogen phosphate / Monohydrogen phosphate ion; pKa = 6.86 Acetic acid / Acetate ion; pka = 4.76
A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H₂C6H6O6] = 5.5 X 10-5 M, [HC6HO6¹¹] = 3.5 X 104 M, and K₂ = 8.00 x 10-5 ? everything is based upon the acid dissolving in water: H₂C6H6O6 + H₂O HC6H6O6¹¹ + H3O+1 [ |][ Ka = [ solve for [H3O+¹] then put in the numbers Ka [ [H3O+¹] = [ [H3O+¹] = pH = -log a. H30+1 b. OH-1 h. HCzH3O2 i. C₂H3O₂-¹ = c. H₂C6H6O6 q. 3 r. 0.5000 s. 5.5 X 10-5 x. 5.5 x 10-² dd. 0.7100 ] y. 0.7000 z. 1.60 x 10-5 ee. 1.26 x 10-5 ff. 4.901 ( d. HC6H606¹¹ j. H₂S k. HS-1 t. 3.5 X 10-4 -1 e. HSO3¹¹ 1. S-² X( m. HX f. SO3² n. X-1 g. H₂SO3 o. 1 p. 2 W. 1.11 x 10-8 u. 8.00 x 10-5 v. 1.75 x 10-6 aa. 1.143 x 105 bb. 0.4900 cc. 1.104 x 10-5 gg. 7.93 hh. 4.942 ii. 4.957
A buffer was created using ascorbic acid and sodium ascorbate. What is the pH of the buffered solution if at equilibrium [H2C6H6O6] = 5.5 X 10-5 M, [HC6H5061] = 3.5 X 10-4 M, and Ką = 8.00 x 10-5 ? everything is based upon the acid dissolving in water: H2C6H6O6 + H20 HC6H601 + H3O*1 Ka solve for [H30+1] then put in the numbers Ka [ [H3O+' : %3D [ [H3O*'] = %3D pH = - log a. H30*1 b. OH-1 c. H2C6H6O6 d. HC6H6061 е. HSO31 f. SO3? g. H2SO3 h. HC2H3O2 i. C2H3O21 j. H2S k. HS-1 I. S2 m. HX n. X-1 О. 1 р. 2 q. 3 r. 0.5000 s. 5.5 X 10-5 t. 3.5 X 10-4 u. 8.00 x 10-5 v. 1.75 x 10-6 w. 1.11 x 10-8 х. 5.5 х 10-2 у. О.7000 z. 1.60 x 10-5 aа. 1.143 х 10-5 bb. 0.4900 сс. 1.104 х 10-5 dd. 0.7100 ее. 1.26 х 10-5 ff. 4.901 gg. 7.93 hh. 4.942 ii. 4.957
What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in sodium lactate [CH3CH1OH2COONa or NaC3H5O3]?For lactic acid, Ka = 1.4 * 10-4.
You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC₂H₃O₂] + [C₂H₃O₂⁻] = 0.250 M) at pH 3.50. How many mL of 1.000 M NaOH must you add in order to change the pH to 5.23? Acetic acid has a pKa of 4.74.

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If this biomolecule was placed into a buffer at a pH of 5.0 in a charged environment would it move towards the postive or negative terminal? H3N-CH- C NH–CH C -NH–CH OH CH2 CH3 CH2 CH2 C-OH Oit is neutral so would not move ○ positive ○ negative I CH2 CH2 NH3