A 0.3147-g sample of a primary-standard grade Na2C2O4 was dissolved in dilute H2SO4 and titrated with 31.67 mL of dilute KMnO4: 2 MnO4- + 5 C2O42- + 16 H+ → 2 Mn2+ + 10 CO2(g) + 8 H2O Calculate the molarity of the KMnO4 solution.
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A 0.3147-g sample of a primary-standard grade Na2C2O4 was dissolved in dilute H2SO4 and titrated with 31.67 mL of dilute KMnO4:
2 MnO4- + 5 C2O42- + 16 H+ → 2 Mn2+ + 10 CO2(g) + 8 H2O
Calculate the molarity of the KMnO4 solution.
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- Five white, 500-mg uncoated ascorbic acid (AA) tablets with an average weight of 0.6152-g were pulverized in a mortar. A sample of the powdered ascorbic acid weighing 0.4700-g was placed in an iodine flask and was dissolved in 50-mL H2SO4 then 5-g of KBr was added to the resulting solution. The solution was titrated with 47.81-mL of 0.09640 N STD. KBrO3 to reach a faint yellow endpoint then 3-g KI and 5-mL Starch TS. The blue color solution is then titrated with 2.73-mL of 0.09123 N STD. Na2S2O3 to reach the disappearance of the blue iodostarch complex. MW: KBrO3 = 167.0 ; KIO3 = 214.0 ; Na2S2O3 = 158.11 ; C6H8O6 = 176.12 Compute the milligrams of pure AA per tablet from the assay. 293.3 mg 502.5 mg None of the choices 383.9 mgThe solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?A 0.5000 g primary standard sodium oxalate (Na2C204, FW=134.00 g/mol) was dissolved in 50 mL of 1 M H2SO4 and required 21.00 mL of the titrant, potassium permanganate (KMnO4, FW=58.03 g/mol) to reach the end point. Calculate the molarity of the titrant *Identify which served as the reducing agent in the titration. * Identify which served as the oxidizing agent in the titration. * Identify the specific name of the redox ti trimetric method used. * Identify the (a) appropriate indicator in t he titration and (b) its type.
- Five white, 500-mg uncoated ascorbic acid (AA) tablets with an average weight of 0.6100-g were pulverized in a mortar. A sample of the powdered ascorbic acid weighing 0.4610-g was placed in an iodine flask and was dissolved in 50-mL H2SO4 then 5-g of KBr was added to the resulting solution. The solution was titrated with 46.73-mL of 0.0152 M STD. KBrO3 to reach a faint yellow endpoint then 3-g KI and 5-mL Starch TS. The blue color solution is then titrated with 2.78-mL of 0.1047 M STD. Na2S2O3 to reach the disappearance of the blue iodostarch complex. MW: KBrO3 = 167.0 ; KIO3 = 214.0 ; Na2S2O3 = 158.11 ; C6H8O6 = 176.12 Compute the milligrams of pure AA per tablet from the assay. None of the choices 349.7 mg 264.3 mg 462.7 mgAn impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate: the molar analytical concentration of K3Fe(CN)6. the weight/volume percentage of K3Fe(CN)6. ppm Fe(CN)6
- The ethyl acetate concentration in a alcoholic solution was determined by diluting a 10.00 mL sample to 100.00 mL. A 20.00 mL portion of diluted solution was refluxed with 40.00 mL of 0.04672 M KOH. Ater cooling, the excess OH2 was back-titrated with 3.41 mL of 0.05042 M H2SO4. Calculate the amount of ethyl acetate (88.11 g mol) in the original sample in grams.3. A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the end point. Report the purity of the Na2CO3 sample.1. 2MnO4— + 5C2O42— + 16H+ 2Mn2+ + 10CO2 + 8H2O A solution of KMnO4 was prepared and 50.99 mL was used to completely titrate 0.5355 g of pure Na2C2O4. What is the concentration of the KMnO4 solution? Na2C2O4 = 134.00 g/mol 2. Titration of the I2 produced from 0.2645g of primary standard KIO3 required 45.36mL of sodium thiosulfate. Calculate the concentration of the Na2S2O3 in M. IO3- + 5I- + 6H+ --> 3I2 + 3H2O I2 + 2S2O32- --> 2I- + S4O62- KIO3 mw = 214.001g/mol
- A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard Method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the end point. Report the purity of Na2CO3sample.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.A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Describe the preparation of the following reagents: 100 mL of 1.0M stock EDTA solution. 0 L of 0.010 M EDTA solution from the stock EDT solution. 0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only).