The amino acid glycine is often used as the main ingredient of a buffer in biochemical experiments. Based on the pKavalues for glycine, in what pH ranges can glycine be used as an effective buffer?In a 0.1M solution of glycine at pH = 9.0, what fraction of glycine has its amino group in the NH form?What volume of 5MKOH must be added to 1L of 0.1M glycine at pH = 9 to bring its pH to 10.0 ?

In a 0.1 M solution of glycine at pH 9.0, the amino group of glycine can exist in two forms: as NH₂…

Answered: The amino acid glycine is often used as…

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...

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3.Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2-Tris or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 x 10^-6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1L of a pH 7.90 buffer? g
A chemist titrates 50.0 mL of a 0.4629 Methylamine (C₂H-NH₂) solution with 0.1652 MHNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO3 solution added. pH = 0 X Ś
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 4.98? Acetic acid has a pKa of 4.74.
How many moles of sodium acetate and acetic acid are required to prepare 1 liter of a buffer, pH 5.0, which is 0.1M in total available acetate (dissociated and undissociated)? Acetic acid has a pKa of 4.74.
Urjant
Kk.362.
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.
3. On the following titration curve label the equivalence point and the pka(s). pH 12.0 10.0 8.0 6.0 4.0 2.0 0.0 0.0 Titration Curve for an Amino Acid 0.5 1.0 OH (equivalents) 1.5 2.0 2.5 3.0
A physician wishes to prepare a buffer solution at pH = 3.82 that efficiently resists changes in pH yet contains only small concentrations of the buffering agents. Determine which one of the following weak acids, together with its sodium salt, would probably be best to use: m-chlorobenzoic acid, Ka= 1.04 × 10-4 ; p-chlorocinnamic acid, Ka=3.89 × 10-5 ; 2,5-dihydroxybenzoic acid, Ka = 1.08 ×10-3 ; or acetoacetic acid, Ka= 2.62 × 10-4 . Explain.
5
A 25.0 mL sample of a 0.1900 M solution of aqueous trimethylamine is titrated with a 0.2375 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C. pH after 10.0 mL of acid have been added = pH after 20.0 mL of acid have been added = pH after 30.0 mL of acid have been added =
HEPES ((4-(2-hydroxyethyl)-1-piperazine ethane sulfonic acid) is a commonly used cell culture buffer with a pKa of 7.5. If you need to prepare 500 mL of 0.2 M HEPES, pH 6.9, how much would you need of the following stock chemicals: 1.0 M HEPES, pH 8.0; 6 M HCI; 6 M NaOH; and distilled H2O?

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