3. Tris(hydroxymethyl)aminomethane [ (HOCH₂)3CNH2, commonly called "Tris" ] is a good non-interacting buffer frequently used with proteins. The pKa value for the protonated form [ (HOCH2)3CNH3 ] is 8.075. The solid salt made with HCl(aq) ("Tris-HCI", the protonated form with a Cl- counter ion) is often utilized to make the buffer - it has a molecular weight of 157.596 g/mole. a. A buffer is made from 15.431 g of solid "Tris-HCI" dissolved in 1000.0 mL of water that contains 0.0462 M NaOH (assume the final volume is also 1000.0 mL). Calculate the pH of this solution. b. Exactly 16.30 mL of 1.761 M HCl(aq) is added to the 1000.0 mL buffer described in part A. What is the new pH?

3. Tris(hydroxymethyl)aminomethane [ (HOCH₂)3CNH2, commonly called "Tris" ] is a good non-interacting buffer frequently used with proteins. The pKa value for the protonated form [ (HOCH2)3CNH3 ] is 8.075. The solid salt made with HCl(aq) ("Tris-HCI", the protonated form with a Cl- counter ion) is often utilized to make the buffer - it has a molecular weight of 157.596 g/mole. a. A buffer is made from 15.431 g of solid "Tris-HCI" dissolved in 1000.0 mL of water that contains 0.0462 M NaOH (assume the final volume is also 1000.0 mL). Calculate the pH of this solution. b. Exactly 16.30 mL of 1.761 M HCl(aq) is added to the 1000.0 mL buffer described in part A. What is the new pH?

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

For HCN, Ka = 4.9 Î 10–10. What is the pH of a buffer solution in which [HCN] = 1.00 M , [KCN] = 0.100 M?
Plz do Asap . !
What is the solubility of AgCN(s) (Ksp = 2.2 × 10⁻¹⁶) in a solution containing 0.35 M H⁺? (Ka for HCN is 6.2 × 10⁻¹⁰.)
Tris(hydroxymethyl)aminomethane is a common base used to prepare buffers in biochemistry. Its Kb is 1.2 x 10−6. What is the pH of a buffer containing 0.01335 M tris (B) and 0.02960 M tris hydrochloride (BH+)?
What mass of NH4Cl (Mw = 53.492 g mol-1) has to be dissolved in 750 mL of 0.25 M NH3 (pKa = 9.26) to prepare a buffer with a pH of 9.72?
Complete the K sp expression for Ag₂CO3. Ksp = 8.46 × 10-12 =
What masses of bromoacetic acid (CH2BrCOOH) and sodium bromoacetate (CH2BrCOONa) are needed to prepare 1.00 L of pH = 2.25 buffer if the total concentration of the two components is 0.200 M? The Ka of bromoacetic acid is 2.0 × 10–3.
Calculate the mass in milligrams (mg). , of silver chromate, Ag-CrO4, that will dissolve in 750 mL of 0.005 M potassium chromate K-CrOa- The Kp of Ag,CrO, is 9.0 x 10-12 b. Find the pH at equivalence point when 75.0 mL of 0.20 M acetic acid, HC2H3O2, is titrated with 0.25 M Ca(OH)2
A buffer with a pH of 9.71 is to be prepared from NH3 and NH4Cl. What ratio of base to saltwould you use? KB(NH3)=1.8x10‒5 (give your answer to 3 sig figs)
Calculate the ratio of KOAc to HOAc required to create a buffer with a pH of 3.92. For HOAc pka =4.74.
buffer consists of 0.30 M ethylamine (C2H5NH2) and 0.40 M C2H5NH3Cl. What is the pH after 5.04 gof HNO3 is added to 2.00 L of the buffer? Kb(C2H5NH2)=5.6×10−4
Can you please answer question 15.90 and all of the sub problems and show all of the steps to the solution