What is the indicator of the end point for the Fajans method? A green fluorescence (B white precipitate (© red precipitate (D red fluorescence
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- Using the term u of KSP experimental procedure the 6 p.m. As you add 5 ml of .004M AgNo to 5ml of .0025M K2CrO4. Is either of these reagents in excess? If so which one?one of the following is correct about Fajans method a. adsorption of Fluorescence on precipitate transfer the color from the precipitate to the solution b. the primary layer of precipitate before reaching the end point has a negative charge c. none of them d. Fluorescence is a basic dye ionized during the titrationThe accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1
- A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-Nickel ion required 11.70 mL of 0.002146 M EDTAWhat is the percentage of NaBr (102.894) in the 1.000 g sample?What is the volume of chloroform required to decrease the concentration of iron (III) in water (50 ml) as [Fe(CNS)6]3- at 20 ppm to 0.1 ppm concentration level in the presence of selective quaternary ammonium or phosphonium salt assuming the distribution ratio of iron (III) complex between chloroform/ water in the presence of the onium and/or phophonium cation =100. What the extraction percentage will be if the volume of the organic solvent is doubled.Is the Cu detectable at a concentration of 0.10 mg/L in Flame-AAS? Please use data given.
- A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA. Calculate mmol Ni in the 50.00 mL aliquot. Calculate mmol Br- in the 50.00 mL aliquot. Calculate the percentage of NaBr (102.894) in the 1.000 g sample.A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br- The liberated nickel ion required 11.70 mL of 0.002146 M EDTA The other 50.00 mL remaining solution was also analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) g) Compute for Eind. h) Compute pBr in the 50.00 mL aliquot. i) Compute for % NaBr ( in the potentiometric technique). j) Calculate the error between the obtained % NaBr fr the EDTA titration technique and the % NaBr from the potentiometric technique.At 25oC the Ksp for PbCl2 is 1.6 × 10–5. Calculate Q for the following: 125.0 mL of 0.0100 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oC
- A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided Determination of the true concentration (ppm Fe) in a water sample using the iron-phenanthroline method. Dilution factor was not taken into account. EX _____ 1ETCalculate the Molar absorptivity constant of a this metal complex solution read at 510 nm using a 50 mm cuvette. C = 1.00 mg/L as Fe Abs = 0.967 (Write answer in whole number, with no decimal and unit)