A cvg.cengagenow.comMy HomeOWLV2 | Online teaching and learning resource from Cen[Review Topics][References]Use the References to access important values if needed for this que... 1 ptsM)1 ptsMWhich of the following aqueous solutions are good buffer systems?1 pts 2reqO 0.32 M nitrous acid + 0.21 M potassium nitrite0.14 M potassium hypochlorite + 0.29 M hypochlorous acid0.22 M perchloric acid + 0.19 M sodium perchlorate0.28 M ammonium nitrate + 0.39 M ammonia0.11 M acetic acid + 0.20 M sodium acetateSubmit AnswerRetry Entire Group8 more group attempts remainingCengage Learning | Cengage Technical Support A cvg.cengagenow.comMy HomeOWLV2 | Online teaching and learning resource from Cenga.Which...1 pts[Review Topics][References]Use the References to access important values if needed for this question.1 ptsMWhich of the following aqueous solutions are good buffer systems?1 pts 2req0.32 M ammonia + 0.34 M calcium hydroxideO 0.34 M barium nitrate + 0.21 M calcium nitrateO 0.16 M acetic acid + 0.15 M sodium acetateO 0.21 M hydroiodic acid + 0.16 M potassium iodideO 0.17 M barium hydroxide + 0.21 M barium chlorideSubmit AnswerRetry Entire Group8 more group attempts remainingCengage Learning | Cengage Technical SupportDD80F7FBF9F3F4F5

Given: Some of the following solutions which can act as a buffer systems To find: which of the…

important values if needed for Which of the following aqueous solutions are good buffer systems? 0.32 M nitrous acid + 0.21 M potassium nitrite 0.14 M potassium hypochlorite + 0.29 M hypochlorous acid O 0.22 M perchloric acid + 0.19 M sodium perchlorate O 0.28 M ammonium nitrate + 0.39 M ammonia O 0.11 M acetic acid + 0.20 M sodium acetate Submit Answer Retry Entire Group 8 more group attempts remaining

important values if needed for Which of the following aqueous solutions are good buffer systems? 0.32 M nitrous acid + 0.21 M potassium nitrite 0.14 M potassium hypochlorite + 0.29 M hypochlorous acid O 0.22 M perchloric acid + 0.19 M sodium perchlorate O 0.28 M ammonium nitrate + 0.39 M ammonia O 0.11 M acetic acid + 0.20 M sodium acetate Submit Answer Retry Entire Group 8 more group attempts remaining

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 56P

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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.
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?
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?
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.)