You are given a diprotic acid H₂A. 10.00 mL of this acid solution of 0.0200 M is titrated with NaOH solution of 0.0213 M (theconcentration is NaOH is standardized by sulfamic acid). pka, = 4.53, pka₂ = 8.59All the following questions are based on the above information.Calculate VelO a. 9.39 mLO b. 18.9 mlO c. 10.00 ml.O d. 9.35 mLCalculate V.2-O a. 15.43 ml.Ob.20.00 ml.O c. 18.78 mlO d. 24.85 mL. What is the pH of the solution after 5.25 ml. of NaOH is added?O a. 4.63O b. 7.00O c. 5.87O d. 8.43What is the most dominant species at 1st equivalence point? H₂A, HA, or A²?0 a. H2AO b. HAOC. A2.What is the pH of the solution at the 1st equivalence point?O a 7.43Ob. 6.23OC. 8.39O d. 6.56

Answered: Image /qna-images/answer/866aa34a-e3ac-43a5-a2df-3fc87f00d738.jpg

You are given a diprotic acid H₂A. 10.00 mL of this acid solution of 0.0200 M is titrated with NaOH solution of 0.0213 M (the concentration is NaOH is standardized by sulfamic acid). pka, 4.53, pka₂ = 8.59 All the following questions are based on the above information. Calculate Vet O a. 9.39 mL O b. 18.9 mL O c. 10.00 mL O d. 9.35 mL Calculate Vez- O a. 15.43 mL O b. 20.00 ml. O c. 18.78 ml. O d. 24.85 ml.

You are given a diprotic acid H₂A. 10.00 mL of this acid solution of 0.0200 M is titrated with NaOH solution of 0.0213 M (the concentration is NaOH is standardized by sulfamic acid). pka, 4.53, pka₂ = 8.59 All the following questions are based on the above information. Calculate Vet O a. 9.39 mL O b. 18.9 mL O c. 10.00 mL O d. 9.35 mL Calculate Vez- O a. 15.43 mL O b. 20.00 ml. O c. 18.78 ml. O d. 24.85 ml.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.97E

See similar textbooks

Similar questions

A 2.500-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.00 mL of 0.798 M HCl. Some acid remains after the treatment of the sample. a Write the net ionic equation for the complete reaction of sodium carbonate with hydrochloric acid b If 28.7 mL of 0.108 M NaOH were required to titrate the excess hydrochloric acid, how many moles of sodium carbonate were present in the original sample? c What is the percent composition of the original sample?
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture of NaHCO3 and Na2CO3 was titrated, what would be the relative sizes of V1, and V2? b. If a mixture of NaOH and Na2CO3 was titrated, what would be the relative sizes of V1 and V2? c. A sample contains a mixture of NaHCO3 and Na2CO3. When this sample was titrated with 0.100 M HCl, it took 18.9 mL to reach the first stoichiometric point and an additional 36.7 mL to reach the second stoichiometric point. What is the composition in mass percent of the sample?
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?