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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 9ALQ: Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA....

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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.150 M NaOH. What was the pH of the solution when the equivalence point was reached?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?
An analytical chemist is titrating 94.2 mL of a 0.4600M solution of dimethylamine ((CH,),NH) with a 0.2300M solution of HNO,. The p K, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 121.9 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH =||
An analytical chemist is titrating 106.9 mL of a 0.8100M solution of dimethylamine ((CH,) NH with a 0.2400M solution of HIO,. The p K, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 413.0 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. dla Round your answer to 2 decimal places. 国 pH = Explanation Check 2021MC Eetinn A Dinhte Desennd Teme oflen Driun Acceeeihility 29 MacBook Air 80 D00 F3 F7 F10 %23 %24 4. & 3 5 7 8 9. E Y P D F G H K
An analytical chemist is titrating 185.1 ml. of a 0.6700M solution of dimethylamine ((CH,), NH) with a 0.6800M solution of HNO,. The p K, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 196.3 ml of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH - 0

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