What was done to ensure that there are no more chloride ions present in the precipitate? (A) Addition of more HCl and testing if the solution becomes acidic B Evaporation of the chloride ions by heating the precipitate in a crucible Filtration using an ashless filter paper to trap the chloride ions on the paper D Addition of AgNO, to the precipitate washings and checking if the washings become cloudy

What was done to ensure that there are no more chloride ions present in the precipitate? (A) Addition of more HCl and testing if the solution becomes acidic B Evaporation of the chloride ions by heating the precipitate in a crucible Filtration using an ashless filter paper to trap the chloride ions on the paper D Addition of AgNO, to the precipitate washings and checking if the washings become cloudy

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

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What was done to ensure that there are no more chloride ions present in the precipitate? (A Addition of AGNO, to the precipitate washings and checking if the washings become cloudy (B Filtration using an ashless filter paper to trap the chloride ions on the paper Addition of more HCl and testing if the solution becomes acidic Evaporation of the chloride ions by heating the precipitate in a crucible
What is the acid/base ratio? Why is it important in the titrimetric process? (Particularly in Double Indicator Titration Method in Determination of % SO3in a Soluble Sample)
ponuq couo buscibics 1o rtol Different aliquot of an unknown ionic solution was tested with different reagent to determine its identity. Aliquot of the unknown precipitated with NaCl and also with NazCO.. What is the probable unknown? Hint: Establish the precipitation reaction of the probable unknown and the reagent Mark only one oval. Silver nitrate mulA Ammonium bromide OPotassium phosphate Barium chlorate hatow n sldulos al bruo
3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution.is precipitated as. Excess of base, next to phenol phthalate (f.f.) indicatorIt is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sampleCalculate its concentration in ppm. (Density of CO2Take it as 1.98 g / L. C = 12, O = 16 g / mol).
A 1.2 g sample of mixture of NaOH and Na COs containing inert impurities s dissolved and titrated cold with 0.5N HCI. With phenolphthalein as indicator the solution turns colorless after the addition of 30.0 ml of the acid. Methyl orange is then added and 12 mL more of the acid is required before this indicator changes color. What is the percentage of NaOH and of Na:CO, in the sample ? 5.
5) 3 L contaminated air 50 mL 0.0116 M in an air pollution analysis Carbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution. as precipitated. Excess of base, next to phenol phthalate (f.f.) indicator It is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sample Calculate its concentration in ppm. (Density of CO2 Take it as 1.98 g / L. C = 12, O = 16 g / mol).
The purpose of adding an excess of the precipitating agent is: 1- Ensure that the sedimentation is complete 2- Get big crystals 3- Purification of the precipitate 4-Prevent pollution
25 mL of a saturated solution of K2Cr2O7 was cooled from 90oC to 50oC, how many moles solid will precipitate from solution?
De to: CaCO3, CaSO,Y 16, What weight of sample which contains 56.15 per cent CI was taken for analysis if the precipitated AgCl weighed 0.5017 g? Ans. 0.2210 g. B. Calculations of Volumetric Analysis
Add 0.3 M AgNO3 to each of the cold sample solutions until AgCl is observed to coagulate. Determine the approximate amount of needed AgNO3 by calculating the volume that would be required if the unknown were pure NaCl.
25) PROVE using calculations and also state whether or not a precipitate will form, (aq., const. Temp.) when 100.0 mL of 0.00250 M BaCl, is mixed with 200.0 mL of 0.00500 M K,SO,. K = 1.10 x 10". sp
Gravimetric Analysis. Please include complete solution, thank you. 4.) A 0.2025 g sample consisting of only BaCl2 and KCl required 20.25 mL of 0.1200 M AgNO3 solution for the quantitative precipitation of chloride. Calculate the %Ba and %K in the sample.