One of the most common buffers used in protein chemistry is a weak base called TRIS (the nitrogen atom of the amino group is thebasic portion of the molecule):Но.-NH2(HOCH2);CNH, = TRIS%3DA biochemist prepares a buffer solution by adding enough TRIS and 12 M HCI to give 1.0 L of a buffer solution that has concentrations[TRIS] = 0.39 M and [TRISH*] = 0.56 M. (pK, of TRIS is 5.91.)(a) Calculate the pH of the buffer solution.pH =i(b) Suppose that 3.3 mL of 12 M HCI is added to 12 L of the buffer solution; calculate the new pH of the solution.pH =i

To calculate pH of a buffer solution , we use Henderson-Hasselbalch equation. For a basic buffer…

A biochemist prepares a buffer solution by adding enough TRIS and 12 M HCl to give 1.0 L of a buffer solution that has concentrations [TRIS] = 0.39 M and [TRISH*] = 0.56 M. (pKp of TRIS is 5.91.) (a) Calculate the pH of the buffer solution. pH = i (b) Suppose that 3.3 mL of 12 M HCI is added to 12 L of the buffer solution; calculate the new pH of the solution. pH = i

A biochemist prepares a buffer solution by adding enough TRIS and 12 M HCl to give 1.0 L of a buffer solution that has concentrations [TRIS] = 0.39 M and [TRISH*] = 0.56 M. (pKp of TRIS is 5.91.) (a) Calculate the pH of the buffer solution. pH = i (b) Suppose that 3.3 mL of 12 M HCI is added to 12 L of the buffer solution; calculate the new pH of the solution. pH = i

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

Consider a buffer made from 255 mL 0.10M HC2H:O2 and 125 mL 0.10 NaC2H:O2. Ka for HC2H3O2 is 1.8 x 105. Choose the true statement. A) Adding 25 mg NaOH (s) will reduce the pH. B) Adding 25 mL water will increase the pH. C) Adding 25 mL 0.0050 M HCI will increase the pH. D) Adding 25 mL 0.0050 M HF will reduce the pH. E) Adding 25 mg NaCl (s) will increase the pH.
A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3HO-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation
You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?
Chemistry (Part -3) =============
do both please as they are the part of the same question..
Determine the pH during the titration of 59.7 mL of 0.392 M hypochlorous acid (K₂ = 3.5×10-8) by 0.392 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 13.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.6 mL of KOH Submit Show Approach Show Tutor Steps
4. A solution prepared to be initially 1 M in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5): (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
Some kidney stones form by the precipitation of calcium oxalate monohydrate (CaCO H₂O, K₁ = 2.3×10). The pH of urine varies from 5.5 to 7.0, and the average [Ca] in urine is 2.6×10 M (a) If the [oxalic acid] in urine is 3.0x10" M, will kidney stones form at pH=5.57 (b) Will they form at pH = 7.0? (c) Vegetarians have a urine pH above 7. Are they more or less likely to form kidney stones?
Consider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d please
A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 5.72) with 20.00 mL of 0.100 M NaOH. This buffer is then divided into 4 equal 15.00 mL parts. If 0.12 mL of a 1.0 M solution of hydrochloric acid is added to one of these 15.00 mL portions of the buffer, what is the pH of the resulting solution?