Suggest a method for the quantitative determination of calcium chloride in the Calcex preparation (hexamethylenetetramine + calcium chloride): A) Argentometry B) Acid-base titration in aqueous media C) Acid-base titration in non-aqueous media D) Complexometry
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9. Suggest a method for the quantitative determination of calcium chloride in the Calcex preparation (hexamethylenetetramine + calcium chloride):
A) Argentometry
B)
C) Acid-base titration in non-aqueous media
D) Complexometry
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- (b) AGNO3 test : Red precipitate formed , which dissolved in dilute HNO3 BaCl2 test : Yellow precipitate formed , which dissolved in dilute HCI Organic solvent test : The decane layer remained almost colorless after treatment with chlorine water Anion present_ (c) AGNO3 test : Yellow precipitate formed , which did not dissolved in dilute HNO3 BaCl, test : No precipitate formed Organic solvent test : The decane layer turned reddish-brown Anion present_(3). Write short notes on displacement titration with suitable example.The substance to be analyzed – is deep-pink colored, highly soluble in water salt. Reaction with NH; gives blue-colored precipitate, which can be dissolved in NH3 surplus accompanied by dirty-yellow colored solution formation. After precipitation of cation by "sodium carbonate drawing out" method, supernatant was independently treated by silver nitrate solution and barium chloride solution (in acid medium in both cases) – any precipitation hasn't been observed. Addition of antipyrin in acid medium changes color to red. What kind of substance is this? Co(NO3)2 CuCl2 Co(CH;COO), FeSO4
- Chromium (III) ion was complexed with EDTA and determined via back-titration. Given the following data, compute for %CrCl3(MM=158.35) in a 2.63 g sample. Conc. of EDTA titrant: 0.0103 MVolume used: 5.00 mLConc. of Zn2+ back titrant: 0.0112 MVolume used: 1.32 mLExplain why in Mohr's method neutral medium should be used in titration of AgNO3?Example (3) :- The Kinehics of hy droly sis of ethyl acetate was Studied in presence Hel by titrating th. reaction Solubon with standard basegmand ( NaoH) at 25 é , the tesults were as foll ows of o.05 M 120 2400 3500 24.36 25.85 2어.32 31.72 Calcutate the fate Constant,what is The order readion ? slafek
- 1. The color of Na,CO3 solution on adding Bromo cresol green indicator changes from to in absence and excess of HCl respectively. (A Yellow; Blue (B) Blue; Yellow Green; Yellow D) Yellow; GreenDetermination of Chloride lon by the Mohr Method Introduction: Objectives: Methods & Materials: Discussion and Conclusion 1. What is the role of chromate ions in chloride determination? 2. Why pH range is important in chloride determination? 3. Would the analytical results by the Mohr method for chlorides be higher, lower or the same as the true color value if any excess of indicator were accidentally added to the sample? Why?A cyanide solution with a volume of 12.99 ml was treated with 30.00 ml. of Ni" solution (containing excess Nit) to convert the cyanide into tetracyanonickelate(): 4 CN + Ni?+ Ni(CN) The excess Nit was then titrated with 11.96 ml. of 0.01357 M ethylenediaminetetraacetic acid (EDTA): Nit + EDTA Ni(EDTA)- Ni(CN) does not react with EDTA. If 39.40 ml. of EDTA were required to react with 30.65 ml. of the original Nit solution, calculate the molarity of CN in the 12.99 mL cyanide sample. 0.12055 (CN = Incorvect
- 1. A 2.2g methyl paraben (mEq of 0.152) was assayed using 50 ml of Sodium Hydroxide, 1.250 N and it consumed 31 ml to of 1.100N sulfuric acid to titrate the excess. In the blank, 42ml of the same acid solution was consumed. What is the percentage purity of Methylparaben? 2. If 25 ml of HCI solution required 26.25 ml of 0.0952N sodium hydroxide in a titration, what volume of the solution would produce 0.2867g of AgCl? (determine the N of acid solution, then use it for the volume that will react with AgCl) 3. A hydrochloric acid solution has AgCl titer of 0.1265, what is its Na2CO3 titer. ( determine the normality of acid using titer value of AgCl, then determine titer value of sodium carbonate) 4. Determine the weight of pure urea in a 500 mg sample if 15.35 ml of 0.4967N NaOH were required in the titration after the ammonia from the sample had been distilled into 50.0 ml of 0.4861N H2SO4.The indicator phenolphthalein may be regarded as a weak monobasic acid. Explain briefly why the indicator is coloured pink when the solution in which it is present has excess of alkali.Chromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.