Review I Constants I Periodic TableA 130.0-mL buffer solution is 0.100 M in NH3and 0.135 M in NH, Br.You may want to reference (Pages 781-791)Section 17.2 while completing this problem.Part AWhat mass of HCI can this buffer neutralize before the pH falls below 9.00?Express the mass in grams to three significant figures.m= .0023SubmitΨΕ ΑΣΦΑX Incorrect; Try Again772=Previous Answers Request AnswerSubmitPart BIf the same volume of the buffer were 0.270 M in NH3 and 0.390 M in NH, Br.what mass of HCI could be handled before the pH falls below 9.00?Express the mass in grams to three significant figures.VG ΑΣΦFOX ?Request Answer?88

Answered: Image /qna-images/answer/d396b505-a43e-40ea-8040-30cb94a66548.jpg

Review | Constants I Periodic Table A 130.0-mL buffer solution is 0.100 M in NH3 and 0.135 M in NH, Br. You may want to reference (Pages 781-791) Section 17.2 while completing this problem. Part A What mass of HCI can this buffer neutralize before the pH falls below 9.00? Express the mass in grams to three significant figures. m- .0023 Submit Part B 15. ΑΣΦ X Incorrect; Try Again 772 = Previous Answers Request Answer Submit If the same volume of the buffer were 0.270 M in NH3 and 0.390 M in NH, Br. what mass of HCI could be handled before the pH falls below 9.00? Express the mass in grams to three significant figures. IVE ΑΣΦ Request Answer ? ? 8 8

Review | Constants I Periodic Table A 130.0-mL buffer solution is 0.100 M in NH3 and 0.135 M in NH, Br. You may want to reference (Pages 781-791) Section 17.2 while completing this problem. Part A What mass of HCI can this buffer neutralize before the pH falls below 9.00? Express the mass in grams to three significant figures. m- .0023 Submit Part B 15. ΑΣΦ X Incorrect; Try Again 772 = Previous Answers Request Answer Submit If the same volume of the buffer were 0.270 M in NH3 and 0.390 M in NH, Br. what mass of HCI could be handled before the pH falls below 9.00? Express the mass in grams to three significant figures. IVE ΑΣΦ Request Answer ? ? 8 8

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 26QAP: You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio...

See similar textbooks

Similar questions

A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
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.
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.)
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
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.
8-94 Suppose you wish to make a buffer whose pH is 8.21. You have available 1 L of 0.100 M NaH2PO4 and solid Na2HPO4. How many grams of the solid Na2HPO4 must be added to the stock solution to accomplish this task? (Assume that the volume remains 1 L.)
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?