A 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).
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- Nickel bis-dimethylglyoximate complex was deposited with a weight of (4.869g) with the filter paper from the base medium from adding (10ml) of hot DMG to a salt of nickel chloride at weight (0.78g), find the percentage of nickel ion. Note that the weight of the filter paper (1.30g). At.Wt.: Ni= 58.69 g/mol, C= 12 g/mol, O=16 g/mol, H=1 g/mol, N=14 g/molNickel 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 100, 0mL containing Zn^ 2+ was treated with 50.0 of 0.0500 M EDTA complex all the Zn^ 2+ and leave excess EDTA in solution. The excess EDTA was then back titrated, requiring 10.00 ml of 0.0500 M Mg^ 2+ was the concentration of Zp^ 2+ original solution ? (Marks)
- A 25.00-mL sample containing Ni2+ was treated with 25.00 mL of 0.5000 M EDTA to complex all the Ni2+ and leave excess EDTA in solution. The excess EDTA was then back titrated, requiring 7.11 mL of 0.450 M Zn2+. What was the concentration of Ni2+ in the original solution (keep 4 SF)?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 mLA 25.00-mL sample containing Fe3+ was treated with 10.00 mL of 0.036 7 M EDTA to complex all the Fe3+ and leave excess EDTA in solution. The excess EDTA was then back titrated, requiring 2.37 mL of 0.0461 M Mg2+. What was the concentration of Fe3+ in the original solution?
- The molar absorptivity for cobalt and nickel complexes with 2,3-quinoxalinedithiol are 3.64x104L/M-cm for Co at 510nm, 5.52x103L/M-cm and 1.24x103L/M-cm for Co at 656nm and 1.75x104L/M-cm for Ni. A 250mg soil sample that was collected near an industrial metal-processing plant is dissolved, and masking agent is added to avoid interference from other metals present. Color is developed by adding the complexing agent and the sample is diluted to 100.00ml. The absorbance at 510nm is 0.517 and at 656nm it is 0.405 in a 1.00cm cell. Calculate the weight percent of Co and Ni in the soil.A 0.60004g sample of Ni/Cu condenser tubing was dissolved in acid and diluted to 100.0mL in a volumetric flask. Titration of both cations in a 25.00mL aliquot of this solution required 45.81mL of 0.05285M EDTA. Mercaptoacetic acid and NH3 were then introduced; production of the Cu complex with the former resulted in the release of an equivalent amount of EDTA, which required 22.85mL titration with 0.07238M Mg2+. Calculate the percentages of Cu (At. Mass = 63.55) and Ni (At. Mass = 58.69) in the alloy. Please provide the complete solution.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?
- A 25.00 mL sample containing Fe3+ was treated with 10.00 mL of 0.03676 M EDTA to complex all the Fe3+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 2.37 mL of 0.04615 M Mg2+. What was the concentration of Fe3+ in the original solution in ppm Fe3+?When I was a boy, I watched Uncle Wilbur measure the iron content of runoff from his banana ranch. He acidified a 25.0-mL sample with HNO3 and treated it with excess KSCN to form a red complex. (KSCN itself is colorless.) He then diluted the solution to 100.0 mL and put it in a variablepathlength cell. For comparison, he treated a 10.0-mL reference sample of 6.80 3 1024 M Fe31 with HNO3 and KSCN and diluted it to 50.0 mL. The reference was placed in a cell with a 1.00-cm pathlength. Runoff had the same absorbance as the reference when the pathlength of the runoff cell was 2.48 cm. What was the concentration of iron in Uncle Wilbur’s runoff ?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 M Volume used: 5.00 mL Conc. of Zn2+ back titrant: 0.0112 M Volume used: 1.32 mL Answer: 0.221%