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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.calculate weight of AgCl when added excess of AgNOs to 0.75g of BaCl2 if M.wt AgCl=143.3 and M.wt BaCk=208.3 AgNO3+ BaClz + BaNOsA scientist wants to check the fuel used in a failed experiment by doing a saponification analysis. He added equal amounts of excess KOH to a blank solution and a solution containing 1.25 g of the fuel. He titrated it with 0.5 M HCl titrant. The results are the following: ml HCl sample blank Vi .8 2.4 Vf 24.8 42 Show the solutions:1. Saponification number (SN) of the oil sample?2. The main component of the oil sample is a diglyceride, calculate the MW of the sample.
- A 0.05002 gram sample of methyl amine (CH3NH2: MW = 31.07 g/mol; Kb = 4.35 x 10-4) was mixed with 100.0 mL of HCl. Calculate the molar concentration of the acid if 5.55 mL of 0.1057 M KOH was needed to back-titrate the unreacted acid.What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?400 mg of a butter sample was heated and some water was added. After shaking and filtration 10 ml 0.2 M Ag* solution, some HNO3 and a few drops of Fe* solution were added to the filtrate. The excess Ag+ in the filtrate was titrated with 01. M standard SCN solution. If the volume of SCN at the equivalence point was 15 mL, calculate the mass percent of NaCl (FW = 58.5 g/mol) in the butter sample
- Oxalic acid (H2C2O4) is present in many plants. If 25.6 mL of 0.0200 M KMnO4 is needed to titrate a 2.75 g sample of plant extract to reach the equivalence point, what is the mass percent of oxalic acid (H2C2O4) in the sample? 2 MnO4- + 16 H+ + 5 C2O42- → 2 Mn2+ + 10 CO2 + 8 H2O2. An analysis for borohydride ion is based on its reaction with Ag+: BH4 - + 8Ag+ + 8OH- -> H2BO3 - + 8Ag(s) + 5H2O The purity of a quantity of KBH4 to be used was established by diluting 3.213 g of the material to exactly 500.0 mL, treating a 100.0-mL aliquot with 50.00 mL of 0.2221 M AgNO3, and titrating the excess silver ion with 3.36 mL of 0.0397 M KSCN. Calculate the percent purity of the KBH4 (53.941 g/mol).2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution.
- All arsenic in the mineral containing 20 g of arsenic is dissolved by converting it into As3+. Calculate the percentage of arsenic in the mineral since the solution is titrated with 43.8 mL of decinormal KBrO3 solution.Potassium permanganate solutions may be standardized by titrating against primary standard sodium oxalate: 2MnO4- + 5C2O42- + 16H+ → 2Mn2+ + 10CO2 + 8H2O. What is the molarity of the KMnO4 solution if 43.80 mL of the KMnO4 is required to titrate 0.2168 grams of Na2C2O4?A sample of freshly precipitated and filtered silver chloride weighs 459.0 mg. If 1.00 % of the silver chloride becomes photo decomposed, what is the precipitate’s weigh?