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…

Organic Chemistry

9th Edition

ISBN:9781305080485

Author:John E. McMurry

Publisher:John E. McMurry

Chapter20: Carboxylic Acids And Nitriles

Section20.3: Biological Acids And The Henderson–hasselbalch Equation

Problem 5P: Calculate the percentages of dissociated and undissociated forms present in the following solutions:...

See similar textbooks

Similar questions

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?
4
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
Payalben
c32
What is the pH of 500mL of a buffer solution of HC3H5O3 0.0570M and C3H5O3Na 0.0275M? Ka of HC3H5O3 = 1.9x10^-5
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.
HA E→ H* +A° d) A solution of an unknown acid has a Pka of 4.4. Calculate the concentration of the undissociated molecules (HA) if a solution of this acid has a pH of 3.2 (Assume that the concentration of Ht ions and A ions are equal).

SEE MORE QUESTIONS

Recommended textbooks for you

Organic Chemistry

Chemistry

ISBN:

9781305080485

Author:

John E. McMurry

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9781305080485

Author:

John E. McMurry

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:

9781285869759

Author:

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

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