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How do you calculate the nominal of Na2S2O3 of the solution?
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- If you prepared a solution of KOH by weighing out 4.750 g of solid KOH that had a purity of 84.6 % and then diluted this to a final volume of 1 L in a volumetric flask, what would be the % mass of KHP in an unknown sample with 0.555 g of mass if it required 20.34 mL of KOH titrant to reach the endpoint? PLEASE show yourHow to prepare these solutions? 250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals 250 mL 0.10 M NaOHNOTE: Use the 1.0 M NaOH prepared250.0 mL standard 2500 ppm Cu(II) stock solutiona. Weigh and dissolve appropriate amount of Cu(NO3)2·5H2O crystals in enough distilled water.A 1.5000-g sample of cereals was analyzed for nitrogen using the Kjeldahl procedure. The receiving flask contained 69 mL of 0.02 M HCl. After the ammonia was collected, the solution was titrated with 0 M NaOH, requiring 11.72 mL to reach the methyl red endpoint. Calculate and percent protein in the sample (f=5.70). Ans. in 3 SFs
- 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.Use the following atomic masses (in g/mol): Mg = 24.31; H = 1; S = 32.06; O = 16; Na = 23; Cl = 35. 45; Ca = 40.08; C = 12.01; N = 14.01; Mg = 24.31 5.A sample of Chlorpheniramine Maleate (99.82%) weighing 0.502g was assayed by non-aqueous titrimetry and was found to be equivalent to 22.2mL of perchloric acid. Calculate for the normality of perchloric acid. Each mL of 0.1N perchloric acid is equivalent to 19.54mg of Chlorpheniramine Maleate.Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. Consider that the burette was completely filled to the 0 mL mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 21.2 mL C. 21.3 mL D. 22.7 mL 2. What is the unknown weight (grams) in the problem? Your Answer:
- Prepare 100.00 mL of a solution with ALL the following chemicals into together; CHEMICALS PROVIDED solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations needed in the 100mL solution FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.Calculate the volume in milliliters of 0.362 M KOH necessary to titrate 28.38 mL of 0.279 M diprotic sulfuric acid, H2SO4, to a phenolphthalein end-point. Report the answer to a precision of 2 decimal places.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.
- 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.Chemistry What is the percentage purity of a sample of impure oxalic acid dihydrate if a sample weighing 0.2003 gram requires 29.30 mL of permanganate solution, of which 1.000 mL ≈ 0.006023 g iron?An analyte solution was prepared using 1.1278 g of a diprotic acid and 25.0 mL of distilled water. A 5.0 mL aliquot was then taken and diluted to 50.0mL. During titration, it required 19.4 mL of a 0.0356 M standardized NaOH solution to reach the end point. a.) What is the molarity of the undiluted analyte solution? b.) What is the molecular weight of the diprotic acid?