Chemistrycreate an anion flow chart without using heat CationsNa", Pb2, Ag*, Ni*, Cr³*, Zn²*, Mg*First do Na"flame testKeep track of anydescriptions. (e.g. Ni3*is green)Then add sourceSupernatant (solution)of Cl (e.g. HCI)Solid precipitate i.e. ppt or PNi2", Cr*, Zn2", Mg*PbCl2, AgClHot HOTry adding stuff to see whathappens!! (Follow your lab manual)SolutionSolidPb2+, ClAgCl(white)or NalPbl2 pptVeryyellowNazSO4PBSO4white pptFigure 4

Answered: create an anion flow chart without…

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create an anion flow chart without using heat

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.18QAP

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Six iron tablets containing FeSO4.7H2O were dissolved in 100-ml of 0.1M HNO3 with gentle heating. All of the Fe2+ is converted to Fe3+ by the strong oxidizing conditions. After the solution had cooled to room temperature , 2.5-ml of 35wt% NH4OH was added. The precipitate Fe2O3-xH2O that was filtered weighed 0.345g. Thermogravimetric analysis of the crude product showed a 10.5% weight loss . A. How many waters of hydration were in the precipitate B. How much iron is present in each tablet
A chemist received different mixtures for analysis with the statement that they contained NaOH, NaHCO3, Na2CO3, or compatible mixtures of these substances, together with inert material. From the data given, identify the respective materials, and calculate the percentage of each component. 1.000g samples and 0.2500N HCl were used in all cases. (A) For Sample W: With PP, 24.32ml was used. A duplicate sample required 48.64ml with MO. (B). For Sample X: The addition of PP caused no color change. With MO, 38.47ml of the acid was required. (C). For Sample Y: To cause a color change in the cold with PP, 15.29ml of the acid was necessary, and an additional 33.19ml was required for complete neutralization. (D) For Sample Z: The sample was titrated with acid until the pink of PP disappeared; this process required 39.96ml. On adding an excess of the acid, boiling, and titrating back with alkali, it was found that the alkali was exactly equivalent to the excess acid added.
Suppose you have a soil that is made up of 10% organic matter with CEC = 200 cmol/kg, 40% kaolinitewith CEC = 10 cmol/kg, and 50% vermiculite with CEC = 100 cmol/kg.1- Calculate the overall CEC of the soil by taking a weighted average of the three soil components.2- What percentage of the overall CEC is contributed by the organic matter? How does that numbercompare to the 10% of the soil itself that is organic?
For Indirect Iodometric Analysis of Copper... ~0.0896g KIO3 necessary to consume 350mL of 0.1 M Na2S2O3, Na2S2O3 is stored in an amber glass bottle until ready for use. Primary Standard KIO3 has 2g of KI, 50mL of DI water, and 10 mL of 1.0M HCl is added then immediately titrated with Na2S2O3 until medium yellow or straw... then 5mL of starch indicator is added and titrated again until blue black color turns clear. Unknown CuO use 1.2G of Unknown, 20mL of HNO3 heated until sample dissolved, 25 mL of DI water added and boiled until clear light blue color, after cooling 1:1 NH3 added (~34.47 mL of NH4OH reagent) until permanent deep blue color amine complex, 2g of NH4HF2 added and swirled until dissolved, 3 g of KI is added then titrated immediately with Na2S2O3 until brown color of iodide is nearly gone (brown milk color), 2 g of KSCN and 3 mL of starch indicator is then added with titration continuing until disappearance of new blue black color. 1. Na2CO3 is often added to thiosulfate…
For Indirect Iodometric Analysis of Copper... ~0.0896g KIO3 necessary to consume 350mL of 0.1 M Na2S2O3, Na2S2O3 is stored in an amber glass bottle until ready for use. Primary Standard KIO3 has 2g of KI, 50mL of DI water, and 10 mL of 1.0M HCl is added then immediately titrated with Na2S2O3 until medium yellow or straw... then 5mL of starch indicator is added and titrated again until blue black color turns clear. Unknown CuO use 1.2G of Unknown, 20mL of HNO3 heated until sample dissolved, 25 mL of DI water added and boiled until clear light blue color, after cooling 1:1 NH3 added (~34.47 mL of NH4OH reagent) until permanent deep blue color amine complex, 2g of NH4HF2 added and swirled until dissolved, 3 g of KI is added then titrated immediately with Na2S2O3 until brown color of iodide is nearly gone (brown milk color), 2 g of KSCN and 3 mL of starch indicator is then added with titration continuing until disappearance of new blue black color. 4. Why is the starch indicator solution…
A 50.00mL sample with BaCl2 was diluted to 650 mL. Aliquots of 100.00 mL of this solution were analysed using Mohr and Volhard methods. The following data were obtained. Volhard method: Volume of AgNO3 = 100mL; Volume of KSCN = 18.25mL Mohr Method: volume of AgNO3: sample = 27.80mL (blank) = 0.30mLWhat is the %BaCl2 using Mohr and Volhard Method. Concentration of KSCN: 0.04000M Concentration of AgNO3: 0.03000M
An acid solution containing 2 per cent by mass of NaNO3, and an unknown concentration of HNO3 is used to regenerate a strong acid resin. After sufficient acid had been passed over the resin for equilibrium to attained, analysis showed that 10 per cent of resin sites were occupied by sodium ions. What was the concentration of HNO3 in the solution, if its density were 1,030 kg/cu.m.?
Nickel bis-dimethylglyoximate complex was deposited with a weight of (2.721g) with the filter paper from the base medium from adding (10ml) of hot DMG to a salt of nickel chloride at weight (0.4g), find the percentage of nickel ion. Note that the weight of the filter paper (0.78g).
A sample of steel (0.506 g) was digested in acid and the solution made up to 100 cm3 with deionised water. Aliquots (25.0 cm3) of this solution were transferred into two volumetric flasks (100 cm3) labelled A and B. Flask A was made up to volume with deionised water. To flask B was added 10.0 cm3 of a 260 ppm standard solution of Mn2+ which was then also made up to volume with deionised water. The following absorbance results were obtained: Solution A = 0.356, Solution B = 0.578. Use these results to calculate the percentage (% w/w) of manganese in the steel sample.
Solution for 0.105g of the K3[Fe(C2O4)3] (MW= 437.2 g/ mol) were dissolved in sulfuric acid and got rated with 9 mL of 0.028M KMn04. What is the experimental weight percent of oxalate in the sample?
Q1. Dissolved 0.273 grams of pure sodium oxalate (Na,C,O.) in distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMNO, solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H; C;O.) with 0.1024 N. Calculate the normlity of KMN0.. Note that the molecular weight of sodium oxalate (Na,C,O.) = 134 and its equivalent weight = 67
A 1.000-gram sample of NaOH (39.997 g/mol) which has been exposed to the air for some time (NaOH will adsorb water and CO2 from the ambient air) is dissolved in water and then diluted to 500.00 mL. 100.0 mL of this solution required 38.60 mL of 0.1062 M HCl to be titrated to the endpoint (~pH 3). A second 100.00 mL portion is treated with excess BaCl2 and then diluted to 250 mL and filtered. 200 mL of the filtrate required 29.62 mL of HCl to titrate to the (~pH 8-9) endpoint. Calculate the mass percentage of NaOH and Na2CO3 (105.9898 g/mol) in the original sample. The adsorbed CO2 is converted to Na2CO3. The Ksp for BaCO3 (s) is 2.58 x 10-9.