Discuss the advantage and disadvantage of Wijs method of iodine value determination. What non-titrimetric method can be used to determine the iodine value of edible oil? Discuss its basic principles and general methods involved.
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Discuss the advantage and disadvantage of Wijs method of iodine value determination. What non-titrimetric method can be used to determine the iodine value of edible oil? Discuss its basic principles and general methods involved.
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- 2.413 g sample contains Na2CO3, NaHCO3 and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO3 and Na CO in sample (Na CO =106.0 g/mol, NaHCO =84.02 g/mol)A 10.00 mL sample containing 8.00 g/L of a mixture of KCI and NaCl was titrated with 0.10 M standard solution of AgNO3; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). 1. O0.0033 2. O0.0800 3. O0.0083 4. O0.0337Titration of an oxalate sample gave the following percentages: 15.30 %, 15.59 % , and 15.57 % 1. Calculate the Average
- An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled to 15°C, treated with 2 drops of Pp indicator and titrated with 1.058 N H2SO4 requiring 6.8 ml to render the solution colorless. Upon adding 2 drops of MO and continuing the titration, 16.5 ml more of the acid were needed to complete the analysis. What is the quantitative composition of the sample? MW: NaOH = 40.0, Na2CO3 = 106.0, NaHCO3 = 84.01A series of solutions containing NaOH, Na.CO, and NaHCO, alone or in compatible combination, was titrated with o.1202 needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate the mass in milligrams of each solute per milliliter of solution. M HCI. Tabulated below are the volumes of acid (2) (1) (а) 22.42 (Ъ) 15.67 (c) 29.64 (d) 16.12 (е) о.00 22.44 42.13 36.42 32.23 33.333Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be the normality of the iodine in order that each ml of titrant represents 1/2% As2O3 in the sample (Answer: 0.0809 N show full solution please)
- Write measurement of Carbon dioxide evolution during respiration of germinating seeds by the Titration methodCaustic 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?Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of commercial bleaching solution titrated ?
- Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Moles of OCl– in the diluted bleach titrated. ?A sample of alfalfa meal weighing 2.0 g is analyzed by Kjeldahl method for the percentage of nitrogen. The liberated NH3 is caught in a solution of H3BO3, and 8.23 ml of HCl are required in the subsequent titration. A sample of pure (NH4)2SO4 (132.12) weighing 0.61 g is treated with excess NaOH and the liberated NH3 (17.04) is also caught in H3BO3. The resulting solution requires 20 ml of the acid for titration. Calculate the percentage of protein in the sample using 6.25 as the factor.Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the volumetric flask). 10ml Initial Burette Reading. 14.80 Final Burette Reading 25.60 Volume of Na2S2O3 used in the titration (mL). 10.80 Moles of Na2S2O3 used in the titration. 1.71 Moles of S2O3–2 used. 1.66 Moles of I2 initially present in titration mixture 0.83 Moles of NaOCl in the diluted bleach titrated. 0.415 Volume of bleach titrated. 1ml Mass of NaOCl in commercial bleach titrated. ?