Question 6 of 36RetryA buffer solution contains dissolved C6H5NH2 andC6H5NH3CI. The initial concentration of C6H5NH2 is 0.50M and the pH of the buffer is 4.20. Determine theconcentration of C6H;NH3* in the solution. The value ofKb for C6H5NH2 is 3.8 x 10-10.12NEXT >Let x represent the original concentration of C6H5NH3* in the water. Based on the givenvalues, set up the ICE table in order to determine the unknown.C6H;NH2(aq) +H20(1)ОН (ад)+ CgH;NH;*(aq)Initial (M)0.50Change (M)Equilibrium(M)-1.6 x 10 10Incorrect, 2 attempts remainingYour Initial concentration for C,H5NH3* is incorrect. Revisit the problem statement to determine the initial concentration of acidor base. Also, make sure that your values are in the correct concentration units, not mass or moles!Your Change in concentration for C6H5NH2 is incorrect. In this problem, you should use the given pH to determine theconcentration of H3O* or OH at Equilibrium as appropriate. From there, you should be able to determine the Change of eachspecies, which is the difference between the Equilibrium and Initial concentration. Recall that pH = -log([H3O*]) and that[H;O*][OH¯] = 1 × 10-14%3DYour Change in concentration for OH" is incorrect. In this problem, you should use the given pH to determine theconcentration of H30* or OH at Equilibrium as appropriate. From there, you should be able to determine the Change of eachspecies, which is the difference between the Equilibrium and Initial concentration. Recall that pH = -log([H3oʻ) and that[H;O*][OH] = 1 × 10-14

A buffer solution is formed by the dissolution of weak acid and its pH and pKa values should be…

A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 × 10¯10. 2 3 NEXT > Let x represent the original concentration of C6H;NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H5NH2(aq) + H2O(1) OH (aq) + C6H5NH3*(aq) Initial (M) 0.50 Change (M) Equilibrium |(M) -1.6 x 10-10 II

A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 × 10¯10. 2 3 NEXT > Let x represent the original concentration of C6H;NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6H5NH2(aq) + H2O(1) OH (aq) + C6H5NH3*(aq) Initial (M) 0.50 Change (M) Equilibrium |(M) -1.6 x 10-10 II

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
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.
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? 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.)
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?
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.)
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.
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.
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.