2. Concentration of metal ion. Absorbance of metal ion in solution 0.316 Concentration of metal ion from the calibration curve (mol/L) 0.084 Concentration of metal ion in the original sample corrected for dilution (mol/L) Show your calculations to account for the dilution of the original sample.
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- To determine the percent purity of a sample containing iron(II) ammonium sulfate; Suggest , 2 different methods for iron(II) ion. Explain in detail what errors may occur in the methods. (volhard method, gravimetric analysis, kjeldahl, etc.) Percentage content: 1-100% ; the solution concentrations to be used are 0.01-0.1M; Take the volumes of solution to be used between 1-50 mLCalculate the saturation indices of the solutions describe below and classify each as undersaturated, supersaturated, or in equilibrium. Saturation state with respect to: Anhydrite (CaSO4) [Ca2+] = 0.00002 mM [SO42-] = 25 mM “Amakinite” (Fe(OH)2) [Fe2+] = 0.1 mM; [OH-] = 0.0001 mM Siderite (FeCO3) [Fe2+] = 3 mM; [CO32-] = 10 mMCaustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?
- Determine the percentage of iron in a sample of limonite from the following data:weight of sample = 0.5000g volume of KMNO4 added 50.0mL ; 1.00mL Kmno4 = 0.0005507 g fevolume of FeSO4 used for back titration 8.00mL ; 1.00mL FeSO4= 0.008950 g FeOMW: Fe= 55.85 FeO= 71.84A 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Show the clear and complete solutionA 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.
- Calculate the molarity of the nickel solution. From the following data calculate the normalities of the acid and base solutions: weight of pure Na2CO3 = 0.2448 g; volume of acid = 43.65 mL ; volume of base used in back titration = %3D 0.84 mL ; 1.000 mL of base = 0.982 mL of acid. Reaction: CO, + 2H* → H2CO3What is the percentage of Nickel in an ore if, when analyzed by the cyanide method, 20.00mL of KCN solution (containing 1.00mmol of AgNO3 per milliliter) are used? Wt of sample used = 0.2500gA 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 = 16.00
- A limestone sample weighing 400 mg was dissolved in acid treated with excess sodium oxalate. The solution was made basic and the resulting calcium oxalate was filtered, washed and redissolved in dilute acid. This solution required 14.0 mL of 0.00865 M KMnO4. What is the % Ca of the limestone. CaC2O4(s) + 2H+ ⇌ Ca2+ + H2C2O45H2C2O4 + 2MnO4- + 6H+ ⇌ 10CO2 + 8H2O + Mn2+A sample of an iron ore was prepared for Fe3+ analysis as following: 3.4g of the sample was added anddissolved in acid environment then diluted to 250 mL using volumetric flask. After that, 10 mL of the resultingsolution was transferred by pipet to a 50-mL volumetric flask and continue to be diluted. The scientists foundout that this solution gives the concentration of Fe3+ as 2.3 mg/L. Find the weight percentage of Fe3+ in theoriginal sample.A student withdraws 3.00Ml of supernate from a saturated solution of KHC8H4O4 at room temp (22C). This sample was titrated to the henolphthalein endpoint and 12.85mL of 0.0997 M NaOH was required A similare tiration was done at 22C for a saturated solution of KHP in 0.500 M KCl. The withgrawn supernant was 5.00mL. The volume of titrant (0.0997M NaOH) used was 11.75. a) calculate the % decrease in solubility by using this equation %decrease = [HC8H4O4]water - [HC8H4O4]sat'd KCl /[HC8H4O4]water