The table below shows a summary of precipitation indicator methods used in titrimetricanalysis. Complete the table by filling in the missing information (I – VI -Precipitateat EndpointEnd-pHMethod AnalyteТуреMechanismIndicatorpointColorrangeChromateRed-(1)CI & BrDirectComplexationNeutralAg:Cro.(Cro.?)brownIndirect1. AgCI2. FESCN?Volhard CI & Ag*(1II)(Backtitration)(IV)Acidic(VI)Weak acidNeutral -Fajan(11)Adsorption(V)dye (E.g.FIO')RedAcidic

Precipitation titration is a kind of titration in which precipitate is formed during the titration…

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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...

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1a) complete the balanced overall ionic equation for the mixing of these two solutions. 2Na+(aq) + 2I-(aq) + Pb2+(aq) + 2NO-3(aq)---> 1b) write the net ionic equation for the mixing of sodium iodide and the solution of lead (2) nitrate. 1c) Complete and balcne the overall ionic equation for lead (2) nitrate dissoliving in water.
A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.
The molar solubility of barium phosphate in a 0.102 M barium nitrate solution is М.
A solution contains 1.19×102 M ammonium carbonate and 1.39x102 M sodium sulfide. Solid nickel(II) nitrate is added slowly to this mixture. What is the concentration of sulfide ion when carbonate ion begins to precipitate? [sulfide] =| M
A 1.00 gram sample of anhydrous cerium sulfate was dissolved in water. Barium nitrate solution was then added until no further precipitation occurred. The precipitate was filtered from the solution then dried and was found to weigh 1.41 g. Determine the formula of the cerium sulfate. Encom calt is hydrated
A solution contains 1.44×10-2 M sodium carbonate and 1.08×102 M ammonium sulfide. Solid manganese(II) nitrate is added slowly to this mixture. What is the concentration of sulfide ion when carbonate ion begins to precipitate? [sulfide] = M
Chemistry If 110.0 mL of 0.0030 MNa2SO4(aq) is saturated with CaSO4, how many grams of CaSO4 would be present in the solution? [Hint: Does the usual simplifying assumption hold?] Express your answer using two significant figures. This answer not 0.07 0.084, 0.09
What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?
The titration of 0.314 g of potassium hydrogen phthalate (KHP) requires 13.16 mL of a NaOH solution. What is the molarity of the NaOH solution?
7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)True
A student weighs a sample of potassium hydrogen phthalate (KHP) to prepare a primary standard for a titration. She later discovers that the KHP was contaminated with sugar. To determine the amount of KHP in the mixture, she takes 4.678 g4.678 g of the mixture and make a 100.0 mL100.0 mL solution. The student then titrates 10.00 mL10.00 mL of this solution with a 0.1030 M0.1030 M sodium hydroxide solution. She finds that 15.15 mL15.15 mL of the NaOHNaOH solution is needed to reach the end point.
You are trying to determine the percentage of acetic acid in vinegar by titrating a sample of the vinegar with a standardized NaOH solution. Why is bromcresol green not a good choice for an indicator for this titration? If you do use bromcresol green as an indicator, will your result for the percentage of acetic acid in vinegar be too high or too low? What would be a better choice for an indicator for this titration? Why is your choice better?

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The table below shows a summary of precipitation indicator methods used in titrimetric analysis. Complete the table by filling in the missing information (I- V -