When a 8.000 g of mineral ore sample containing Sn(CO,), (238.7 g/mol) and other inert material was reacted with excess HCl solution and the liberated CO, was bubbled through an excess solution of Ca(OH)2 (74.0 g/mol); the mass of precipitated CaCO, (100.0 g/mol) was 0.6200 g. The percentage Sn(CO,)2 in sample is? 1 054.97 % 2 09 25 % 3 0 18.30 % 4. 08.35%
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- The concentration of CO in the air can be determined by passing a known volume of air through a tube containing I2O5, resulting in the formation of CO2 and I2. I2 is removed from the tube by distillation and collected in a solution containing excess KI, producing I3-. I3- is titrated with a standard solution of Na2S2O3. A 4.79 L air sample was sampled as described here, requiring 7.17 ml of 0.00329 M Na2S2O3 to reach the endpoint in a typical analysis. If the density of the air is 1.23×10^-3 g/ml, what is the amount of CO in the air in ppm? (CO: 28 g/ml)The concentration of CO in air is determined by passing a known volume of air through a tube that contains I2O5, forming CO2and I2. The I2 is removed from the tube by distilling it into a solution that contains an excess of KI, producing I3-. The I3-is titrated with a standard solution of Na2S2O3. In a typical analysis a 4.79-L sample of air is sampled as described here, requiring 7.17 mL of 0.00329 M Na2S2O3 to reach the end point. If the air has a density of 1.23 × 10–3 g/mL, determine the parts per million CO in the airTo determine , by gravimetric analysis, the concentration of barium ions (Ba2+) in a given solution, 25.00cm3 of it are pipetted into a beaker and an excess of dilute sulphuric acid is added to it. The precipitate then obtained (BaSO4) is filtered, dried and weighed. The mass of the precipitate is found to be 1.167g Calculate the concentration of barium ions in the solution? (only 2 decimal places). _________Mol/L
- The concentration of arsenic in an insecticide can be determined gravimetrically through its precipitation as MgNH4AsO4. After the formation of the precipitate, it must be ignited for total conversion to Mg2As2O7, which is then cooled and weighed. Considering that a sample of 1,627 g of the insecticide produced 106.5 mg of Mg2As2O7, determine the% (m/m) As2O3 in the insecticide. Given the molar masses: Mg2As2O7 = 310.447 g / mol and As2O3 = 197.841 g / mol1,5419 g of magnetite (Fe3O4) ore; in concentrated HCL to form a mixture of Fe + 2 and Fe+3it's unraveling. By adding HNO3 to it, all Fe+2 s are upgraded to Fe+3. And the addition of FE+3 s NH3,with Fe (OH)3, precipitating into. The sediment is weighed as 0.8525 g in the form of Fe2O3 after the necessary operations. Calculate the percentage of Fe3O4 in the sample.The arsenic in a 1.223-g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, as 40.00 mL 0.07891 M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag+ in the filtrate and washings from the precipitate was titrated with 11.27 mL of 0.1000 M KSCN; the reaction was Ag+ + SCN- → AgSCN(s) Calculate the percent As2O3 in the sample.
- A student weighed out 3.5689g of unknown nickel salt and carried out the gravimetric analysis in order to determine the % nickel in the unknown sample. The mass of one of the two bis(dimethylglyoximate) nickel(11) precipitates that was filtered was 0.1570g. How many moles of Ni 2+ are in the precipitate?The arsenic in a 1.010 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and exactly 40.00 mL of 0.06222M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag in the filtrate and in the washings from theprecipitate was titrated with 10.76 mL of 0.1000MKSCN; the reaction wasAg+ + SCN-→ AgSCN(s) Calculate the percent AsO3 in the sample.A sample containing NaCl, NaBr, and inert materials weighs 1.000 g. With excess AgNO3 it gives a precipitate of AgCl and AgBr, which weighs 0.5260 g. By heating this precipitate in a current of Cl2 gas, the AgBr is converted to AgCl and the resulting precipitate then weighs 0.4260 g. What is the %NaCl and %NaBr present in the original sample?
- To determine the amount of magnetite, Fe3O4 in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl to obtain a mixture of Fe2 + and Fe3 +. After HNO3 is added to oxidize Fe2 + to Fe3 + and diluted with water, Fe3 + is precipitated as Fe (OH) 3 by adding NH3. 0.8525 g of pure Fe2O3 is obtained by filtering, rinsing and burning the precipitate. Calculate the percentage of Fe3O4% in the sample. (Fe = 55,847g / mol, O = 15,999g / mol)A sample containing NaCl, NaBr, & inert material weighs 1.000 g. Excess of AgNO3 gave a whiteprecipitate consisting of only AgCl and AgBr which weighs 0.5260 g. By heating the precipitate in a currentof Cl2 gas, the AgBr (187.78 g/mol) is converted to AgCl (143.32 g/mol) and the precipitate weighs 0.4260g. Find the % NaCl (58.44 g/mol) and % NaBr (102.909 mol) in the original sample.0.5366 g of an KHP sample of unknown purity was massed. The sample was dissolved in approximately 100 mL of distilled, degassed water and indicator was added. The end point was reached after 21.35 mL of 0.09854 M NaOH solution was titrated into the solution. What is the percentage of KHP in the original sample?