Assuming that the concentration of concentrated HCI is 10 M, estimate approximately how muchconcentrated HCI will be required to bring the pH of the 1.0 M Tris solution to 7.5, using the followinginformation.log [conjugate base][Iconjugate acid]H/H equation:pHpKa%3D+The total molarity of Tris in the solution is made up of:[Tris (conjugate base form) + Tris (conjugate acid form)]i.e. in this example,[Tris-c.base] + [Tris-c.acid] = 1.0Mpka of Tris ~8.1You wish to make 200 mL of Tris-CI buffer

The amount of acid and base, in terms of molarity, is calculated as shown below.…

Assuming that the concentration of concentrated HCI is 10 M, estimate approximately how much concentrated HCI will be required to bring the pH of the 1.0 M Tris solution to 7.5, using the following information. H/H equation: pH log [conjugate base] [Iconjugate acid] pKa %3D + The total molarity of Tris in the solution is made up of: [Tris (conjugate base form) + Tris (conjugate acid form)] i.e. in this example, [Tris-c.base] + [Tris-c.acid] = 1.0M %3D pKa of Tris 8.1 You wish to make 200 mL of Tris-Cl buffer

Assuming that the concentration of concentrated HCI is 10 M, estimate approximately how much concentrated HCI will be required to bring the pH of the 1.0 M Tris solution to 7.5, using the following information. H/H equation: pH log [conjugate base] [Iconjugate acid] pKa %3D + The total molarity of Tris in the solution is made up of: [Tris (conjugate base form) + Tris (conjugate acid form)] i.e. in this example, [Tris-c.base] + [Tris-c.acid] = 1.0M %3D pKa of Tris 8.1 You wish to make 200 mL of Tris-Cl 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

A chemist titrates 210.0 mL of a 0.3206M ammonia (NH3) solution with 0.3768 M HCl solution at 25 °C. Calculate the pH at equivalence. The pK, of ammonia is 4.75. 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 HCl solution added. pH = 0 X
Nitesh
An analytical chemist is titrating 117.9 mL of a 0.4500M solution of dimethylamine ((CH3)₂NH) with a 0.4400M solution of HNO3. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 129.2 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 ? 国 h
KHP(aq) + NaOH(aq) -> H2O (l) + KNaP(aq) 1. If we forgot to add the phenolphthalein indicator, why would we be unable to determine the NaOH molarity? 2. If we used a sample of KHP with too big a mass, what experimental problem would we run into? 3. Why does adding a small amount of DI water not affect the calculation of the NaOH molarity?
An analytical chemist is titrating 208.8mL of a 0.7500M solution of methylamine CH3NH2 with a 0.5600M solution of HNO3 . The pKb of methylamine is 3.36 . Calculate the pH of the base solution after the chemist has added 236.8mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
A chemist titrates 160.0 mL of a 0.3445 M pyridine (C-H5N) solution with 0.8552M HNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of pyridine is 8.77. 6 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. E pH = 0 X 5 OL 9 L
An analytical chemist is titrating 137.4 mL of a 0.2300M solution of methylamine (CH3NH2) with a 0.1600M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 223.0 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.
Payalben
An analytical chemist is titrating 129.9mL of a 0.5200M solution of hydrazoic acid HN3 with a 0.2100M solution of NaOH . The pKa of hydrazoic acid is 4.72 . Calculate the pH of the acid solution after the chemist has added 241.9mL 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.
A chemist titrates 150.0 mL of a 0.0676M dimethylamine ((CH,) NH) solution with 0.4402M HBr solution at 25 °C. Calculate the pH at equivalence. The pK, of dimethylamine is 3.27. 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 HBr solution added. pH = Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibity MacBook Air
I need the answer as soon as possible
Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > 5 A solution of phenol (HC H₂O) is prepared by dissolving 0.385 g of phenol in 2.00 L of H₂O. The solution has a pH = 6.29. Fill in the ICE table with the appropriate value for each involved species o determine the unknown concentrations of all reactants and products. H_O*(aq) + Initial (M) Change (M) Equilibrium (M) 1 HC,H,O(aq) + 5 H₂O(1) 2 C_H,O(aq)