3. The K, for the weak base methylamine is 4.4 x 10*. A buffer solution is prepared bydissolving 0.326 moles of methylamine, CH3NH2, and 0.504 moles of the salt CH;NH3C1in 1 L of solution.a. Use the Henderson-Hasselbach equation to compute the pH of this buffer solution.b. 0.074 moles of the strong base KOH is added to the buffer solution above. Assumingthat the addition of the base does not change the volume of the solution, compute theOH concentration at equilibrium and the pH of this mixture.

The Henderson Hasselbalch equation for basic buffer is given as :

Answered: 3. The K, for the weak base methylamine…

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

4) A buffer solution is made from 135 mL of 0.395 M in HC2H3O2 and 115 mL 0.345 M NaC2H3O2 (the Ka of acetic acid is 1.79 x 10-5). a. Determine the pH of the initial buffer solution. b. What is the buffering range of this solution? c. What is the buffering capacity of this solution? d. What is the maximum volume of 2.00 M HCl solution you can add this buffer before it is no longer effective?
5. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC₂H3O2 mixed with 15.00mL of 0.3000M NaOH c. 22.50mL of 0.2000M NH3 mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HClO₂ mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH₂ mixed with 25.00mL of 0.1500M HCI
17. Determine the pH of the resulting solutions when the following reagents are mixed. a. 20.00mL of 0.2500M HCI mixed with 35.00mL of 0.2250M NaOH b. 18.00mL of 0.3500M HC2H;O2 mixed with 15.00mL of 0.3000M NaOH 22.50mL of 0.2000M NH, mixed with 25.00mL of 0.1000M HCI d. 25.00mL of 0.1000M HCIO, mixed with 25.00mL of 0.1000M KOH e. 15.00mL of 0.1000M CH3NH2 mixed with 25.00mL of 0.1500M HCI
1. calculate the pH of a solution obtained by mixing 30.4 mL of 0.03 M HCL with 31.4 mL of o.1 M HNO3 solution 2.A given weak acid has a pKa of 8.27. Calculate the percent ionized in 0.34 M of the weak acid. 3. Calculate the pH of 0.021 M Sr(OH )2 PLEASE DO ALL THREE
Calculate the pH of each of the following solutions a. 0.10 M propanoic acid, CH3CH2COOH, Ka = 1.3 x 10-5 b. 0.10 M sodium propanoate, NaCH3CH2COO. c. A mixture containing 0.10 M propanoic acid and 0.10 M sodium propanoate d. Calculate the pH after 0.020 mole of HCl is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate e. Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of a solution that contains 0.10 M propanoic acid and 0.10 M sodium propanoate
Hh.129.
A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka’s for KHP are 1.12 x 10-3 and 3.90 x 10-6. a. Calculate the pH of this solution before adding any NaOH. b. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? c. Calculate the pH of the solution after 100. ml of NaOH have been added.
6. Consider a solution that has 0.00500 M HCl and 0.100 M HF. Ka of HF = 7.2x10-4. a. What is the pH of this solution? b. Suppose the solution was like that in A but also had 0.1 M HOI. (i.e. total solution was a mix of 0.00500 M HCl, 0.100 M HF, and 0.1 M HOI). Ka of HOI = 2.0x10-¹¹. Does this solution have an appreciably different pH than the solution in part a? Support your answer with relevant calculations. HINT: Work from strongest acid to the weakest acid.
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
Calculate the pH of the buffers prepared in the following ways: a. by mixing 50.00 mL of 0.200 M ammonium nitrate, NH,NO,, with 25.00 mL 0.200 M NaOH b. by neutralizing half of the acid in 100.00 mL of 0.200 M ammonium nitrate solution with 1.0 M NaOH c. by mixing 60.00 mL of 0.400 M sodium formate (NaCHOO) with 40.00 mL 0.360 M HCI d. by mixing 80.00 mL of 1.00 M NH, with 40.00 mL of 1.00 M HCI e. by mixing equal volumes of 1.00 M NH, and 0.50 M HCI
Consider the situation in which 50.0 mL of 0.200 M HNO3 is being titrated with 0.100 M NaOH. Determine each quantity: 3. determine the pH after adding 20.0 mL of base
Consider the titration of 30.00 mL of 0.0500 molar ammonia with 0.0250 molar HCl. a.What is the pH of this solution at the equivalence point?

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