☐ x10bA chemistry graduate student is given 250. mL of a 0.10M methylamine (CH3NH2) solution. Methylamine is a weak base with K₁ =4.4 × 104. What mass ofCH3NH3Br should the student dissolve in the CH3NH2 solution to turn it into a buffer with pH = 10.21?You may assume that the volume of the solution doesn't change when the CH3NH3 Br is dissolved in it. Be sure your answer has a unit symbol, and round it to2 significant digits.G

Answered: Image /qna-images/answer/c2e5df8f-59d6-4687-86b2-8a9c00c13523.jpg

Answered: ☐ x10 b A chemistry graduate student is…

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 buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If [HBrO] is 0.100 M, then what concentration of hypobromite ion is needed to achieve pH = 8.50
What quantity in moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 11.00?
What quantity in moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 10.90?
A chemistry graduate student is given 250. mL of a 0.10M methylamine (CH3NH2) solution. Methylamine is a weak base with K 4.4 x 10 CH3NH2Br should the student dissolve in the CH3NH2 solution to turn it into a buffer with pH = 10.21? What mass of You may assume that the volume of the solution doesn't change when the CH3NH3Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 ☐ x10 X G
How many grams of sodium formate, HCOONa, are required to mix with 1.50 Liters of 0.500 M formic acid, HCOOH, in order to prepare a buffer solution with a pH that equals 4.00? pKa(HCOOH) = 3.74 and MM(HCOONa) = 52.01 g/mol
A chemistry graduate student is given 500.mL of a 0.80M chloroacetic acid (HCH2ClCO2) solution. Chloroacetic acid is a weak acid with Ka = 1.3x10^−3. What mass of NaCH2ClCO2 should the student dissolve in the HCH2ClCO2 solution to turn it into a buffer with pH = 3.08 ?You may assume that the volume of the solution doesn't change when the NaCH2ClCO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A chemistry graduate student is given 100. mL of a 1.20M pyridine (CHN) solution. Pyridine is a weak base with K₁=1.7 × 10¯⁹. What mass of CH₂NHBr should the student dissolve in the CH₂N solution to turn it into a buffer with pH = 4.82? You may assume that the volume of the solution doesn't change when the C5H-NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 Ś
A buffer can be prepared from a weak acid, HA, and it's conjugate base, A⁻. A 1L solution is prepared in which the concentrations are [HA] = 0.1M and [A⁻] = 0.2 M. The pKa of HA is 6.4. What is the pH of this solution before and after 50 ml of 1M HCl, a strong acid, is added?
What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer with a pH of 3.10? (Ka for HF is 6.8 × 10⁻⁴)
3. Please solve the following chemistry problem.
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS