Ni content of the steel can be determined by the precipitation gravimetric analysis. For this purpose, 1.000 g of a steel sample is taken and interacted with the concentrated HCI solution. After neutralizing the resulting mixture in the presence of citrate ions, 1% dimethyl glyoxime (DMG) solution is slowly added to precipitate Ni(II) ions as Ni(DMG)2. What is the percentage of nickel in this steel sample, if 0.2269 g of Ni(DMG), (288.93 g/mol) is obtained?
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- An acidic solution of copper (.35 M Cu+2) was treated with KOH until Cu(OH)2 precipitated. At what pH does this occur at?1. Aluminum is determined gravimetrically by precipitating Al(OH)3 and isolating Al½O3. A sample that contains approximately 0.1 g of Al is dissolved in 200 mL of H2O, and 5 g of NH4C1 and a few drops of methyl red indicator are added (methyl red is red at pH levels below 4 and yellow at pH levels above 6. The solution is heated to boiling and 1:1 NH3 is added dropwise until the indicator turns yellow, precipitating Al(OH)3. The precipitate is held at the solution's boiling point for several minutes before filtering and rinsing with a hot solution of 2% w/v NHẠNO3. The precipitate is then ignited at 1000–1100 °C, forming Al>O3. a) Cite at least two ways in which this procedure encourages the formation of larger particles of precipitate. b) The ignition step is carried out carefully to ensure the quantitative conversion of Al(OH)3 to Al203. What is the effect of an incomplete conversion on the %w/w Al? c) What is the purpose of adding NHẠCI and methyl red indicator? d) An alternative…Suppose you wanted to analyze the amount of metal in the alloy. For example, you might want to determine the nickel (Ni2+) content in alloy material. (a) Suppose the nickel had been precipitated from the alloy (2.0980g) using dimethylglyoxime (H2DMG) as an organic precipitating agent and giving a precipitate of complex nickel dimethylglyoxime (Ni(HDGMG)2) weighing 0.2370g. Calculate the percentage weight of nickel (Ni2+) in the alloy sample.
- A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample. NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+A 1.000-g sample of limestone gave a precipitate of Fe2O3 and Al2O3, weighing 0.0800 g. The precipitate of mixed oxides was fused with KHSO4, dissolved in sulfuric acid, and passed through a Jones reductor. The iron was titrated with 20.00 mL of 0.0100 N permanganate solution. Calculate the percentage of FeO and Al2O3 in the limestone (assume all iron present as FeO in the original sample)Suppose you wanted to analyze the amount of metal in the alloy. For example, you might want to determine the nickel (Ni2+) content in alloy material. (a) Using gravimetric analysis, propose precipitating method to analyze nickel (Ni2+) in alloy and write 8 steps required during the precipitation. Also, suggest an appropriate solvent and its ratio dissolve the mixture. Here we recommended using dimethylglyoxime (H2DMG) as an organic precipitating agent.(b) Suppose the nickel had been precipitated from the alloy (2.0980g) using dimethylglyoxime (H2DMG) as an organic precipitating agent and giving a precipitate of complex nickel dimethylglyoxime (Ni(HDGMG)2) weighing 0.2370g. Calculate the percentage weight of nickel (Ni2+) in the alloy sample.
- Can cadmium (II), and mercury (II) be separated quantitatively by precipitation as sulfides from a solution that is 0.15 M cadmium nitrate and 0.10 M in mercuric ions? If possible, what range of sulfide concentration is permissible? Do you expect any interference from the formation of hydroxides of both heavy metals? CdS (144.46); Ksp = 1.0 x 10 ^ -27HgS (232.66); Ksp = 2.0 x 10 ^ -53 HINT: Determine the concentration at which each of the cations start to precipitate out of solution. >Quantitative precipitation means 1/1000 remains in solution.a three step process is required in order to determine the concentration of NO3- in a basic solution: 1) Zinc metal reduces Nitrate ions into ammonia in basic environments2) the ammonia is transferred to a solution with a known excess of HCl3) the unreacted HCL is titrated with NaOH A) write a balanced equation for each process B) a 25.00ml basic Solution containing an unknown concentration of NO3- was treated with zinc metal, the ammonia gas from the reaction was reacted with a 50ml solution of 2.5*10^-3M of HCl, the remaining unreacted HCL was then titrated to the stochiometric point with 28.22ml of 1.5*10^-3 NaOHWhat is the molar concentration of NO3- in the original solution?What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.
- Consider the following reaction. Fe3+ (aq) + SCN (ag) FESCN2*(ag) a) İnitially [Fe3+]=1,0 x 10-3 M and [SCN]= 8,0 x 104 M a solution was prepared. In balance [FESCN2-] = 1,7 x 104 M. Calculate the equilibrium constant Kd.The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O O2. An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HC. The resulting solution was diluted with water, and the iron(III) was precipitated as hydrous oxide Fe,03 .XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,03 (FW = 159.69). Calculate (a) the percent Fe (FW = 55.847) and (b) the percent Fe;04 (FW = 231.54) in the sample.