The Ką of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48 M NAOH. Which of thefollowing is correct for the following two processes?(1) After addresulting solution.ml of N2OH into the above 0.72 M C6H5COOH of 40.0 mL, we have [ C6H5COOH ] = [ C6HSCO0" ] in the(2) After addthe resulting solution.ml of NaOH into the above 0.72 M CGH5COOH of 40.0 mL, we have [ CgHgCOOH ] = [OH" ] inO a. The answer for (1) is 40.0 ml. The answer for (2) is 20.0 ml.O b. The answer for (1) is 20.0 ml. The answer for (2) is 40.0 ml.O. The answer for (1) is 30.0 ml. The answer for (2) is 60.0 ml.d. The answer for (1) is 60.0 ml. The answer for (2) is 30.0 ml.O e. None of the above is correct.

Option C The answer for (1) 30.0 ml and the answer for (2) 60.0 ml

The Ka of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48 M NaOH. Which of the following is correct for the following two processes? (1) After add resulting solution. ml of NaOH into the above 0.72 M C6H5COOH of 40.0 mL, we have ( C6H5COOH ] = [ C6H5COO" ] in the (2) After add ml of NaOH into the above 0.72 M CGH5COOH of 40.0 mL, we have [ C6H5COOH ] = [OH* ] in the resultinn solution

The Ka of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48 M NaOH. Which of the following is correct for the following two processes? (1) After add resulting solution. ml of NaOH into the above 0.72 M C6H5COOH of 40.0 mL, we have ( C6H5COOH ] = [ C6H5COO" ] in the (2) After add ml of NaOH into the above 0.72 M CGH5COOH of 40.0 mL, we have [ C6H5COOH ] = [OH* ] in the resultinn solution

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...

See similar textbooks

Similar questions

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.
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.
Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high purity and is used to determine the concentration of solutions of strong bases by the reaction HP(aq)+OH(aq)H2O(l)+P2(aq) If a typical titration experiment begins with approximately 0.5 g KHP and has a final volume of about 100 mL, what is an appropriate indicator to use? The pKa for HP is 5.51.
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.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
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?
What is [Br-] just as AgCl begins to precipitate when 1.5 M AgNO3 is slowly added to a solution containing 0.050 M Cl- and 0.050 M Br-?