Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02156 M Fe²+ by 0.03517 M EDTA at a pH of 6.00. Thevalues for log Kf and ay can be found in the chempendix.13.00 mLpFe²+19.50 mL=the equivalence point, VepFe²+ =1.58IncorrectpFe2+ =10.31Incorrect6.376Incorrect

Answered: Calculate pFe²+ at each of the points…

Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02156 M Fe²+ by 0.03517 M EDTA at a pH of 6.00. Th values for log Kf and ay can be found in the chempendix.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A student titrates 20.0 mL of solution of Mg(OH)2 with 0.0420 M EDTA. The initial buret reading was…

A: Mole of EDTA added is approximately 6.17 x 10-4 mol

Q: 50.00 ml of a solution containing iron (11) and iron (III) when titrated at pH2.0, 12.50 mL 0.01200…

A: The metal which can get titrated without interfering from others would be Fe3+. The complex…

Q: 4. A 0.584gram sample of a fertilizer was analyzed for its N content by the kjeldahl method, the…

A: analysis of % N and Urea, H2NCONH2

Q: moles

Q: 1. Calculate the pPb^2+ at each of the following points in the titration of 20.00 mL of 0.0200M…

A: EDTA called as ethylenediaminetetraacetic acid is a complexometric indicator consisting of 2 amino…

Q: Determine the pH at the equivalence point for the titration of a 40.0 mL sample of 0.100 MHNO2 by…

A: Given:Concentration of HNO2 = 0.100 MConcentration of KOH = 0.200 MVolume of HNO2 = 40.0 mLpKa of…

Q: For the titration: 30.0mL of 0.150 M NH3 (Kb = 1.8 x 10-5) with 0.250 M HBr Calculate the pH after…

A: For the given titration we have to calculate the pH

Q: Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM…

Q: Calculate the theoretical pH-value for 0.050 M Potassium phosphate (a solution that displays buffer…

A: Answer is explained. Explanation:HCl dissociation: HCl → H⁺ + Cl⁻ The initial concentration of HCl…

Q: The end point of a titration was reached after 22.2 mL22.2 mL of 0.050 M0.050 M disodium EDTA…

A: Given : At the endpoint of the titration : The volume of disodium EDTA=22.2 mL = 22.2/1000 = 0.0222…

Q: Classify the type of elementary step shown below. H H. N-CH3 -I H N-CH3 H

A: The following reaction is an elimination reaction and by eliminating leaving group an alkyne is…

Q: A titration curve is shown below. What is the ratio of A to HA (A:HA) at the lower end of this…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding a small…

Q: In this experiment, the color change from pink/violet to colorless during the titration is caused…

A: A redox titration is a type of titration based on a redox reaction between the analyte and titrant.…

Q: Calculate the equivalence point volumes for a titration of 25.00 mL of 0.060 M HCl and 01.0 M H3PO4…

A: HCl vs NaOH Volume of HCl ( Va ) =25.00 mL Molarity of HCl ( Ma ) = 0.060 M Molarity of NaOH ( Mb…

Q: a) Calculate the pH after 0.0100 mol of H+ ions are added to 0.100L of buffer containing 1.00M…

A: Note: Since you have posted multiple questions, we will provide the solution only to the first…

Q: 0.0500M

A: The objective of this question is to show the equivalence point is reached when the amount of AgNO3…

Q: A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with…

A: The objective of the question is to determine the concentration of Ca2+ and Mg2+ in the solution.…

Q: The chemist performed a titration that follows the equation below. He used 25.00 mL of . sulfuric…

A: The given reaction is: H2SO4 (aq) + 2OH- (aq) →SO42- (aq) + 2H2O (l) The volume of sulfuric acid V1=…

Q: Determine the pH at the equivalence point for the titration of a 40.0 mL sample of 0.100 MHNO2 by…

A: Given: Concentration of HNO2 = 0.100 M Concentration of KOH = 0.200 M Volume of HNO2 = 40.0 mL pKa…

Q: Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02037 M Fe²+by 0.03675 M…

Q: 13.00 mL pFe2+ the equivalence point, V. pFe2+ = 17.50 mL pFe?+

A: The question is based on the complexometric titration of ferrous ions and EDTA. we have to calculate…

Q: Calculate the following points on the titration curve for the reaction of 20.00 mL of 0.1075 M Pb4+…

Q: A 0.3606-g of a weak monoprotic was dissolved in water and then titrated with 0.1040 N KOH solution.…

A: Given - weak monoprotic = 0.3606-g titrated with solutions = 0.1040 N KOH Total…

Question

Calculate pFe²+ at each of the points in the titration of 25.00 mL of 0.02156 M Fe²+ by 0.03517 M EDTA at a pH of 6.00. The
values for log Kf and ay can be found in the chempendix.
13.00 mL
pFe²+
19.50 mL
=
the equivalence point, Ve
pFe²+ =
1.58
Incorrect
pFe2+ =
10.31
Incorrect
6.376
Incorrect

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: introduction

VIEW

Step 2: Ve and conditional formation constant determination

VIEW

Step 3: PFe2+ determination when volume of Fe2+ solution is 13 ml

VIEW

Step 4: PFe2+ determination at equivalence point

VIEW

Step 5: PFe2+ determination at equivalence point

VIEW

Step 6: determination of concentration of Y4- and FeY2- when volume of Fe2+ solution is 17.50 ml

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 7 steps with 5 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

what volume of .65 M strong titrant would be needed to drop pH of a buffer by 0.33 if the buffer was made from 0.0448 moles of pyruvic acid pka 2.55 and 0.0672 moles of the conjugate base pyruvate anion? calculate the pH of the buffer before seeing how much is changing
Calculate pF at the equivalence point of a titration of 20.00 mL of 0.01039 M La (NO3)3 with 0.006338 M NaF.
A Consider the pH titration curve above (pH vs volume in ml). The pk, of the weak base being titrated and the pH of the equivalence point are, respectively: 12 11 10 8 7 5 4 2 1 10 20 30 40 O 2.5 and 4.0 • 5.4 and 4.5 O 11.2 and 5.4 O 11.2 and 4.5 O 4.5 and 5.4 Based on the indicator information above, which of the following indicators could be used successfuly in the titration in Part A? (Select all correct responses. Indicator Colour (low pH – high pH) pK, methyl yellow red-yellow 3.1 methyl orange red-yellow 3.7 bromophenol blue yellow-blue 4.2 bromocresol green yellow-blue 4.7 methyl red pink-yellow 5.1 bromocresol purple bromothymol blue yellow-purple 6.3 yellow-blue 7.0 phenol red yellow-red 7.9 O phenol red cresol red yellow-red 8.3 O bromocresol purple thymol blue yellow-blue 8.9 O methyl yellow thymolphthalein colourless-blue 9.2 O bromothymol blue O thymol blue O thymolphthalein Part C Baseu on the table above, what colour is methyl orange at pH3? Submit Request Answer Part…
Given a 0.100 M solution of anserine at its isoelectric point and ready access to 0.200 M HCl, 0.200 M NaOH and distilled water, describe the preparation of 1 L of 0.0300 M anserine buffered solution, pH 7.20. Volume of stock solution needed = ? mL Volume of HCl needed to adjust the imidazole group = ? mL Volume of HCl needed to titrate the amino group = ? mL Total HCl needed = ? mL
i forgot how to do this pls help soon