Describe a concise step by step lab procedure for preparing a standard aqueous solution containing 3.019 millimolar (mM) of Pb from solid lead nitrate Pb(NO3)2 analytical grade reagent with a high purity of 99.989 %. Show and state the relevant calculations and/or assumptions in each step of the procedure.
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- The Fe content in a water sample from a well was determined by subjecting an aliquot of 25.00ml of sample to treatment with HNO3, excess SCN- and finally a dilution of the treated solution to 50.00mL with distilled water. A 10.00ml aliquot of a 5.97 x 10-4M Fe3 + solution was treated in the same way. It was observed that the color of both solutions was the same when the optical path of the standard solution was 3.04cm and that of the well water sample was 2.61cm. Determine the ppm of Fe in the well water sample.A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.Titarant in Mohr's method is AgNO; solution; KSCN solution; Hg2(NO3)2 solution; NaCl solution
- A sample of Al;(SO.); weighing 7.52-g was dissolved in enough water and diluted to 250.0-mL. 100.0-mL of the dilution was transferred to another flask, 10.0-mL of 0.050M EDTA, 20-ml of buffer solution, 50-mL of alcohol and 2.0-ml dithizone TS were added. The resulting solution required 8.7-mL of 0.031M ZnSO, to reach the endpoint. (Note: Each ml of 0.050M EDTA is equivalent to 16.66-mg Al:(SO.);•18H;0). Compute for the percent purity of the sample.A sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data: Wt of sample = 0.5000g; Vol of AgNO3 added = 35.00ml; M of AgNO3 = 0.1157; Vol of SCN- used for back titration = 14.71ml; M of SCN- = 0.08598; Atomic wts: Ag = 107.87, N = 14.00, Cl = 35.5, O = 16.00Preparation of cpper(1) chloride What color observed for the solution of Na2SO3 in water? What colour observed for solutions of CuCl2.2H2O in water? Which ion is responsible for the colour that is observed in the CuCl2 solution? What is observed when th Na2SO3 solution is added to the CuCl2? Which gas can be smelled when H2SO4 is added to the mixture? What is the colour of the CuCl when it is filtered on Buchner funnel? (before it is exposed to the atmosphere) What is the colour of the CuCl when it is filterd on the Bucher funnel? (before it is exposed to the atmosphere) Does the colour of the CuCl remain the same if you leave it to dry in the atmosphere? Calculate the percentage yields for the experiment
- Preparation of cpper(1) chloride What color observed for the solution of Na2SO3 in water? What colour observed for solutions of CuCl2.2H2O in water? Which ion is responsible for the colour that is observed in the CuCl2 solution? What is observed when th Na2SO3 solution is added to the CuCl2? Which gas can be smelled when H2SO4 is added to the mixture? What is the colour of the CuCl when it is filtered on Buchner funnel? (before it is exposed to the atmosphere)Q7) what is the pH at the equivatent point in the titration of 5 mmol Potassium acid ph thalate dissolved in 100 mel of water and titrat ed with 0.1M NaoH 9 K, = 4 +r56 %3D Ans. : 8.46A Sample Containfng mmol of KNOS is "parsed 6.00 x10-2² mmol of vesay ad z.00x102 mmol af ves@y ad 2.00x1o2 though a cation -excharye Column. the Colculate. volume o.02.00 M NaH of needed to titrete the elwate,
- A sample containing BaCl, 2H,0, KCI and inert material weighed 0.8417 g. After heating the sample at 160°C for 45 min, it weighed 0.8076 g. The sample was then dissolved in water and treated with a slight excess of AgNo,. The resulting precipitate was collected and found to weigh 0.5847 g. Calculate the % Bacl,-2H,0 and % KCI in the sample. 3.Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard cuvette (1.00 cm light path) of 0.382. Calculate the mass of Co(NO3)2 contained in the original 50.0 mL stock solution.(a) Interpret the variation, including the overall trend across the 3d series, of the following values of hydration enthalpies (in kJ mol·'). [Ca(H2O)«]²*: -2468; [Ti(H2O)«J*: -2700; [V(H2O)«]**: -2814; [Mn(H2O)6]**: -2743; [Fe(H2O)«]²+: -2843; [Co(H20)6]**: -2904; [Ni(H2O)c]*: -2986. (b) By making use of LFSE (Ligand field stabilization energy) in tetrahedral and octahedral geometries, predict whether hausmannite mineral (Mn3O4) has a normal spinel or inverse spinel structure. Describe the structure of the mineral in detail.