The pH of a cyanoacetic acid/sodium cyanoacetate buffer in which the concentration of the weak acid component is 0.140 M and the concentration of the conjugate base is 0.070 M is 2.16. Suppose 0.144 g of solid NaOH are added to 100 mL of this buffer solution. What is the pH after the addition? Click here for the table of lonization Constants of Weak Acids. Please enter your answer with 2 decimal places.

The pH of a cyanoacetic acid/sodium cyanoacetate buffer in which the concentration of the weak acid component is 0.140 M and the concentration of the conjugate base is 0.070 M is 2.16. Suppose 0.144 g of solid NaOH are added to 100 mL of this buffer solution. What is the pH after the addition? Click here for the table of lonization Constants of Weak Acids. Please enter your answer with 2 decimal places.

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 61QAP: Each symbol in the box below represents a mole of a component in one liter of a buffer solution;...

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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.
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Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?