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?

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?

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

Give Detailed Solution
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.
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.
The desired pH is 6.4 in creating a buffer system/buffer solution of about 50-60mL. Therefore, a student picks Silicic Acid Si(OH)4, as 1mL of 1M of the acid has a pH of 6.4, which also has a pKa of 9.82. What is the ratio HA/A- and ratio A-/HA-? The buffering capacity will be checked by the addition of 1mL of 1M HCl or 1mL of 1M NaOH and should not change by more than 0.25pH units.
5.) What is K, for an acid whose pK, is 3.78?
The pKa of acetic acid is 4.74. What is the pH of a buffer solution that is prepared from 0.010 M acetic acid (HCHO) and 0.0080 M potassium acetate (KC2H3O2)?
Suppose a biochemist has 10 mL of a 1.0 M solution of a compound with two ionizable groups at a pH of 7.60. She adds 10.0 mL of 1.0 M HCI, which changes the pH to 3.40. The pK, value of one of the groups is pK,= 3.90 and it is known that pK₂ is between 7 and 10. What is the exact value of pK₂? pK₂ = 7.1 Incorrect
The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). Calculate the pH of a saturated solution of Mg3(AsO4)2 in water.
Blood pH = 7.4 and the pKa values of carbonic acid, H2CO3 are 6.35 and 10.33. Calculate the HCO3–/H2CO3 ratio of the carbonate buffer at physiological pH.
Calculate the pH of a 2.00 M Na2CO3 given that the pKa’s of the first and second dissociation of H2CO3 (aq) acid are 6.37 and 10.32, respectively.
Kk.74.
Given the values of K and Kb below, which of the systems given would be most suitable to use to construct a buffer of pH 97 HCOOH, K, = 1.8 x 104 CH3COOH, K3=18x105 H3ASO4. Ka1 = 6.0 x 10, Ka2 = 1.1 x 10, Ka3 = 3 x 1012 C5H5N, Kp = 1,7x10-9 NH3 КЬ - 1.3 х. 10-5 OA H3ASO4/NaH2As04 eB. HCOOH/NAHCOO OC. C5H5N/ C5H5NHCI OD.CH3COOH/KCH3CO0 FOE NH4C/NH3