Q5. a) What is the appropriate value (pay attention for the significant figure) that should breported for the volume of the liquid seen into the burette? (remember the titration video)2223b) Consider the titration of an example of propanoic acid by using the solution of sodium hydroxidof an exact amount. Explain what you attempt to see at the equivalence point (make the comparisorof the quantity of species). (Describe the titration process and draw the necessary diagram. I want tsee all the details).Ka for propanoic acid at 25°C: 1.3 x 10$

a) Given is the image of a burette.

Q5. a) What is the appropriate value (pay attention for the significant figure) that should reported for the volume of the liquid seen into the burette? (remember the titration video) 22 23 b) Consider the titration of an example of propanoic acid by using the solution of sodium hydroxi of an exact amount. Explain what you attempt to see at the equivalence point (make the comparise of the quantity of species). (Describe the titration process and draw the necessary diagram. I want see all the details). Ka for propanoic acid at 25°C: 1.3 x 10s

Q5. a) What is the appropriate value (pay attention for the significant figure) that should reported for the volume of the liquid seen into the burette? (remember the titration video) 22 23 b) Consider the titration of an example of propanoic acid by using the solution of sodium hydroxi of an exact amount. Explain what you attempt to see at the equivalence point (make the comparise of the quantity of species). (Describe the titration process and draw the necessary diagram. I want see all the details). Ka for propanoic acid at 25°C: 1.3 x 10s

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 114CP

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Similar questions

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 bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
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.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
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.