Caustic 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?
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Caustic 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?
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- To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.The fat in a 1.821 g sample of potato chips is extracted with supercritical CO2. After extraction, the residue weighs 1.139 g. What is the fat content (% w/w) of the potato chips?Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. A. How many moles of HCl was added initially to digest the limestone sample? B. How many moles of CaCO₃ is present in the limestone sample? C. What is the purity of the limestone in terms of %w/w CaCO₃?
- An analyst was assigned to work a sample with minerals. This iron-containing sample was analyzed by dissolving a 1.3142g sample in concentrated HCl. The resulting solution was diluted with water and iron (III) was precipitated as the hydrated oxide Fe2O3 xH2O by the addition of HN3. After filtration and washing, the residue was calcined at high temperature to produce 0.5488g of pure Fe2O3 (159.69g / mol). Determine the following:a) the% Fe (55.847 g / mol) and the% Fe3O4 (231.54 g / mol) in the sample.Suppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water. The solution is acidified with 6 M HCl, heated, and an excess of aqueous BaCl2 is slowly added to the mixture resulting in the formation of a white precipitate. 1) Assuming that 0.433 g of precipitate is recovered calculate the percent by mass of SO42− in the unknown salt. 2) If it is assumed that the salt is an alkali sulfate determine the identity of the alkali cation.On the first phase, which is prepared by dissolving some bromine (Br2) in 10 mL of carbon sulfur at constant pressure and 25 ° C, 20 mL of water is added at the same temperature. After waiting for the well-shaken mixture to come to equilibrium, the carbon sulfur and water phases are completely separated and the bromine amounts are determined. It has been experimentally determined that there is 1.29 g of bromine in the carbon sulfur phase and 0.0064 g of bromine in the water phase. a) Partition coefficient of bromine between carbon sulfur and water phases ......................determined as. b) If 2.2 g of bromine were dissolved in carbon sulfide initially at the same pressure and temperature, the mass of bromine passing into the water phase ...................... ...... ..................... (MBr: 79,904 g / mol) Note: enter only required numerical values and units in the spaces in the question.
- On the first phase, which is prepared by dissolving some bromine (Br2) in 10 mL of carbon sulfur at constant pressure and 25 ° C, 20 mL of water is added at the same temperature. After waiting for the well-shaken mixture to come to equilibrium, the carbon sulfur and water phases are completely separated and the bromine amounts are determined. It has been experimentally determined that there is 1.29 g of bromine in the carbon sulfur phase and 0.0064 g of bromine in the water phase. a) Partition coefficient of bromine between carbon sulfur and water phases b) If 2.2 g of bromine were dissolved in carbon sulfide initially at the same pressure and temperature, the mass of bromine passing into the water phase (MBr: 79,904 g/mol)A student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g. Compute for the theoretical % SO3 obtained by the student and the theoretical mass (g) of SO3 that should be obtained by the student using his weighed sampleA student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g.29. Compute for the mass (g) of BaSO4 from the experiment.A) 0.3933B) 0.3393C) 0.3133D) 0.3951E) 0.359130. Compute for the experimental mass (g) of SO3 in grams obtained by the student.A) 0.1439B) 0.1349C) 0.1943D) 0.1394E) 0.359131. Compute for the experimental % SO3 obtained by the student.A) 73.21B) 56.33C) 17.89D) 56.89E) 72.8032. Compute for the theoretical % SO3 obtained by the studentA) 0.3933B) 56.37C) 17.33D) 17.89E) 0.425233. Compute for the theoretical mass (g) of SO3 that should be obtained by the student…