Just looking for assistance with B. Please be neat and detailed. I want to be able to replicate (May assume activity coefficient = 1.0 for simplification in this problem)Citric acid is a triprotic acid (H3L), with acidity constants K₁1 = 10-3.13, K₁2= 10-4.72, and Ka3 = 10-6.33HOcitric acidOHOH(a) Construct a logC-pH diagram using Excel or other similar software toillustrate the speciation of the solution containing 1.0x10-³ M of totalcitric acid. Based upon the speciation diagram, determine the mostdominant species at pH 4 and pH 9, respectively.(b) A solution is prepared by adding 1.0x10-3 M trisodium citrate (Na3L)to pure water. Calculate the equilibrium pH of this solution.

Dissociation of citric acid can be given as,Given:concentration of trisodium citrate = 1.0 x 10-3…

Answered: Calculate the equilibrium pH of this…

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Calculate the equilibrium pH of this solution.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.5QAP

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Just looking for assistance with B. Please be neat and detailed. I want to be able to replicate

(May assume activity coefficient = 1.0 for simplification in this problem)
Citric acid is a triprotic acid (H3L), with acidity constants K₁1 = 10-3.13, K₁2
= 10-4.72, and Ka3 = 10-6.33
HO
citric acid
OH
OH
(a) Construct a logC-pH diagram using Excel or other similar software to
illustrate the speciation of the solution containing 1.0x10-³ M of total
citric acid. Based upon the speciation diagram, determine the most
dominant species at pH 4 and pH 9, respectively.
(b) A solution is prepared by adding 1.0x10-3 M trisodium citrate (Na3L)
to pure water. Calculate the equilibrium pH of this solution.

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A 35 year old male was taken to the hospital with excruciating pain in the lower abdominal area. It was discovered that this patient drank no more than half a glass of water each day over the past week, while drinking at least three cups of black tea on the same days. Additionally, the patient regularly eats very large quantities of spinach. Upon further analysis, it was determined that the presence of Calcium Iodideand Sodium Oxalate may have led to the pain that the patient was experiencing. Determine whether or not kidney stones could be the probable cause of the lower abdominal pain for this patient by answering the following questions (Be sure to show your work for all parts): Assume that Calcium Iodideand Sodium Oxalate are the starting substances (reactants) in the reaction: a. Write a balanced chemical equation describing the formation of kidney stones, using the information in the case study. b. State the names of the products that are produced from this reaction. c.…
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