An analytical chemist is titrating 84.3 mL of a 0.8200M solution of propylamine(C,H,NH,) with a 0.2500M solutlon of HNO,. The p K, of propylamine is3.46. Calculate the pH of the base solution after the chemist has added 307.6 mL of the HNO, solution to it.3.Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.3.Round your answer to 2 decimal places.do国pH =CheckExplanation2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy AccessibilityV 5:39hpBô->Ceescbackspace@#38.9.712tyerWtab%24

This is an example of basic buffer.After the equivalence point all the bases present in the solution…

Answered: An analytical chemist is titrating 84.3…

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 analytical chemist is titrating 84.9 mL. of a 0.2500M solution of hydrazoic acid (HN3) with a 0.7400 M solution of NaOH. The pK, of hydrazoic acid is 4.72. 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.
A chemist titrates 150.0 mL of a 0.5341 M carbonic acid (H,CO,) solution with 0.2213M KOH solution at 25 °C. Calculate the pH at equivalence. The p K, of carbonic acid is 3.60. 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 KOH solution added. pH = | ? %D
Write the chemical formulas of acetic acid and sodium acetate Determine the pH of the following buffer solution that is a mixture of 50.0m/ of 0.144M acetic acid and 55.0m/. of 0.137M sodium acetate. Ka of acetic acid is 1.8 x 105. Determine the pff of the buffer solution in problem #2 after 4.0m/ of 0.25MNaOH is added,
A 50.000 mL aliquot of weak base that has a concentration of 0.285 M will be titrated with 0.684 M HCl. Calculate the pH of of the solution upon the addition of 20.851 mL of HCl. The Kb of the base is 7.5×10-6. Report your answer to the hundredths place. If the difference between moles of analyte and moles of titrant is less than 1x10-4, assume it is at the equivalence point.
An analytical chemist Is titrating 100.6 mL of a 0.7200M solution of ammonla (NH,) with a 0.4000M solution of HNO,. The p K, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 205.4 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initlal volume of the solution plus the volume of HNO, solution added. 3 Round your answer to 2 decimal places. pH = || Check Explanation 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessi hp Ce esc & OC %24
A buffer solution contains 0.302 M NaHSO3 and 0.438 M K2SO3. If 0.0168 moles of hydrochloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydrochloric acid)...
Be sure to answer all parts. Exactly 100 mL of 0.15 M nitrous acid (HNO,) are titrated with a 0.15 M NaOH solution. (a) Calculate the pH for the initial solution. (b) Calculate the pH for the point at which 80.0 mL of the base has been added. (c) Calculate the pH for the equivalence point. (d) Calculate the pH for the point at which 105 mL of the base has been added.
A chemist titrates 110.0 mL of a 0.1235M butanoic acid (HC,H,CO,) solution with 0.0643 M KOH solution at 25 °C. Calculate the pH at equivalence. The pK, of butanoic acid is 4.82. 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 KOH solution added. pH = ] ? %3D
An analytical chemist is titrating 74.8 mL of a 0.7500M solution of propylamine (C,H,NH,) with a 0.2500M solution of HIO,. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 265.9 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. olo pH = I Ar
An analytical chemist Is titrating 108.4 mL of a 0.2200M solutlon of plperidine (C HNH) with a 0.8700M solution of HI0,. The p K, of plperidine Is 2.89. 10 Calculate the pH of the base solution after the chemist has added 15.5 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. alb pH = |] Explanation Check 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility A 6:08 hp 么 -> esc #3 2$ 3. 4. t y e r tab 00
The pH of a bicarbonate-carbonic acid buffer is 5.63. Calculate the ratio of the concentration of carbonic acid (H₂CO3) to that of the bicarbonate ion (HCO3). Be sure your answer has the correct number of significant digits. Note: Reference the pK, of acids at 25 °C table for additional information. [HCO3] [H₂CO3]]
4) A buffer solution with a volume of 72.3 mL is made with 0.00752 of HCHO, and 0.00941 mol NaCHO,. If 0.214 g of HCl is added without changing the volume of the solution, what is the pH of the resulting solution? The pk of formic acid: 3.74.

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