Use the References to access important values if needed for this question. When a 23.5mL sample of a 0.426M aqueous hydrocyanic acid solution is titrated with a 0.303M aqueous sodium hydroxide solution, what is the pH after 49.6mL of sodium hydroxide have been added? pH = 9 more group attempts remaining Use the References to access important values if needed for this question. When a 23.5 mL sample of a 0.426 M aqueous hydrocyanic acid solution is titrated with a 0.303 M aqueous sodium hydroxide solution, what is the pH after 49.6 mL of sodium hydroxide have been added? pH = Submit Answer Retry Entire Group 9 more group attempts remaining

Use the References to access important values if needed for this question. When a 23.5mL sample of a 0.426M aqueous hydrocyanic acid solution is titrated with a 0.303M aqueous sodium hydroxide solution, what is the pH after 49.6mL of sodium hydroxide have been added? pH = 9 more group attempts remaining Use the References to access important values if needed for this question. When a 23.5 mL sample of a 0.426 M aqueous hydrocyanic acid solution is titrated with a 0.303 M aqueous sodium hydroxide solution, what is the pH after 49.6 mL of sodium hydroxide have been added? pH = Submit Answer Retry Entire Group 9 more group attempts remaining

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 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

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A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.