Dino needs to prepare 200.0 mLs of a 0.25M /0.20 M buffer solution that has pH of4.7.To make this buffer solution, Dino has available 0.50 M solutions each of thefollowing:Chemicals..NH3/NH4CI•HCOOH/HCOOKHONH2/HONH3CICH3COOH/NaCH3COO●NH3/NH4CIHONH2/HONH3CHCOOH/HCOOKK₂Which set of conjugate acid - base pairings should Dino select?CH3COOH/NaCH3COO1.78 x 10-55.62 x 10-101.82 x 10-49.12 x 10-9

Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Dino needs to prepare 200.0 mLs of a 0.25M /0.20 M buffer solution that has pH of 4.7. To make this buffer solution, Dino has available 0.50 M solutions each of the following: Chemicals ● ● CH3COOH/NaCH3COO NH3/NH4CI •HCOOH/HCOOK HONH2/HONH3CI Which set of conjugate acid - base pairings should Dino select? ● NH3/NH4CI HONH2/HONH3CI HCOOH/HCOOK Ka 1.78 x 10-5 5.62 x 10-10 1.82 x 10-4 9.12 x 10-⁹ CH3COOH/NaCH3COO

Dino needs to prepare 200.0 mLs of a 0.25M /0.20 M buffer solution that has pH of 4.7. To make this buffer solution, Dino has available 0.50 M solutions each of the following: Chemicals ● ● CH3COOH/NaCH3COO NH3/NH4CI •HCOOH/HCOOK HONH2/HONH3CI Which set of conjugate acid - base pairings should Dino select? ● NH3/NH4CI HONH2/HONH3CI HCOOH/HCOOK Ka 1.78 x 10-5 5.62 x 10-10 1.82 x 10-4 9.12 x 10-⁹ CH3COOH/NaCH3COO

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 33QAP: A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this...

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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?
Water is accidentally added to 350.00 mL of a stock solution of 6.00 M HCI. A 75.00-mL sample of the diluted solution is titrated to pH 7.00 with 78.8 mL of 4.85 M NaOH. How much water was accidentally added? (Assume that volumes are additive.)
A solution of KOH has a pH of 13.29. It requires 27.66 mL of 0.2500 M HCI to reach the equivalence point. (a) What is the volume of the KOH solution? (b) What is the pH at the equivalence point? (c) What is [K+] and [Cl-] at the equivalence point? Assume volumes are additive.
How many grams of HI should be added to 265 mL of 0.215 M HCI so that the resulting solution has a pH of 0.38? Assume that the addition of HI does not change the volume of the resulting solution.
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A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
You have a solution of the weak acid HA and add some HCl 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.
Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution.
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 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?
A solution consisting of 25.00 g NH4Cl in 178 mL of water is titrated with 0.114 M KOH. (a) How many milliliters of KOH are required to reach the equivalence point? (b) Calculate [Cl-], [K+], [NH3], and [OH-] at the equivalence point. (Assume that volumes are additive.) (c) What is the pH at the equivalence point?
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.

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