4. Biochemical experiments frequently utilize a buffer system based on tris- (hydroxymethyl)aminomethane, (HOCH2)3CNH2, which is also called TRIS or THAM. The pKa of the conjugate acid of TRIS, (HOCH2)3CNH3+, is 8.075. What mole ratio of acid-to-base is required to prepare a buffer at the same pH as human blood, pH = 7.4? pob

4. Biochemical experiments frequently utilize a buffer system based on tris- (hydroxymethyl)aminomethane, (HOCH2)3CNH2, which is also called TRIS or THAM. The pKa of the conjugate acid of TRIS, (HOCH2)3CNH3+, is 8.075. What mole ratio of acid-to-base is required to prepare a buffer at the same pH as human blood, pH = 7.4? pob

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

An aqueous solution contains 0.329 M methylamine (CH3NH2).How many mL of 0.305 M perchloric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.700.
What is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium chloride CH3NH2Cl? The Kb for CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.
A buffer solution is formed by adding 0.150 moles of solid strontium acetate, Sr(C₂H₃O₂)₂, to 500.0 ml of 0.400 M acetic acid, HC₂H₃O₂ solution. You may assume that the change in volume is negligible upon addition of the solid.Calculate the pH of the buffer solution.Calculate the pH of the buffer solution after the addition of 7.50 ml of 2.00 M NaOH. Acetic Acid: pKa = 4.75 Ka=1.76E-5 M.w.=60.05 g/mol
propionic acid, ?a=1.34×10−5,Ka=1.34×10−5, 3.00 M sodium propionate, CH3CH2COONa 1. The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 5.00? ( in g) 2. Based on this information, what volume of acid should the student measure to make the buffer solution? (in ml)
What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4Cl) in enough water to form 2.50L of solution. The K, of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBr is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H5O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.
A buffer consists of 0.50 M NaH₂PO₄ and 0.40 M Na₂HPO₄.Phosphoric acid is a triprotic acid (Kₐ₁=17.2X10⁻³, Kₐ₂=26.3X10⁻⁸, and Kₐ₃=34.2X10⁻¹³). (a) Which Kₐ value is most important to this buffer? (b) What is the buffer pH?
An analytical chemist is titrating 145.6mL of a 1.100M solution of hydrazoic acid HN3 with a 0.8100M solution of KOH . The pKa of hydrazoic acid is 4.72 . Calculate the pH of the acid solution after the chemist has added 236.7mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
Calculate the pH of a buffer formed by mixing 85.0 mL of 0.130 M lactic acid, HC3H503, with 95.0 mL of a 0.150 M solution of sodium lactate, NaC3H5O3. The Ka of lactic acid is 1.40 x 10-4.
A 1.50 L buffer solution consists of 0.280 M propanoic acid and 0.139 M sodium propanoate. Calculate the pH of the solution following the addition of 0.065 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The Ka of propanoic acid is 1.34×10^−5.
An analytical chemist is titrating 75.3 mL of a 0.2100M solution of cyanic acid (HCNO) with a 0.8800M solution of NaOH. The p K of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 20.9 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 0
A 1.33 L buffer solution consists of 0.168 M butanoic acid and 0.272 M sodium butanoate. Calculate the pH of the solution following the addition of 0.075 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The ?a of butanoic acid is 1.52×10−5.
An aqueous solution contains 0.386 M dimethylamine ((CH3)2NH).How many mL of 0.379 M perchloric acid would have to be added to 250 mL of this solution in order to prepare a buffer with a pH of 10.800.