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- FeCl3 and MgCl2 solution was prepared by dissolving FeCl3 (AR) and MgCl2 (AR) in distilled water. Secondly, under rapid stirring, NaHCO3 powder was slowly added to the above solution to the desired basicity (B = 1) which had been proved to be the optimal B for turbidity removal. Thirdly, Na2HPO4 (AR) was added to the PFMC solution as a stabilizer ([Na2HPO4]/([Fe] + [Mg]) = 0.08). i. The the chemical equation of the Synthesis. ii How much weight need to put NaHCO3 above solution the desired basicity (B=1) iii. How much weight need to put Na2HPO4 on PFMC solution refering ([Na2HPO4]/([Fe] + [Mg]) = 0.08).Given that the equivalence point volume from the second derivative plot is 7.3429, how many grams of salicylic acid (138.121 g/mol) was synthesized? To determine the yield of the hydrolysis reaction, potentiometric titration was done. NaOH was used as the titrant, and three trials of standardization with KHP yields a titrant concentration of 0.0427 M.In complexometric titration ‘the reaction with analyte should be rapid andcomplete’ give reason with suitable justification for the above statement.
- why is it necessary to test the ph? EXTRME DETAIL PLEASE PROCEDURE To a six inch test tube was added thiamine hydrochloride (0.65 g), followed by water (2mL). The mixture was gently shaken until homogeneous, and then ethanol (7.5 mL)was added. Finally, sodium hydroxide (10%, 1.5 mL) was added and the mixture wasgently stirred to ensure complete mixing.Benzaldehyde (3.8 mL) was then added at room temperature in one portion with gentlestirring. The pH of the resulting reaction mixture was determined and adjusted to >10by dropwise addition of 10% sodium hydroxide.why is it necessary to test the ph? PROCEDURE To a six inch test tube was added thiamine hydrochloride (0.65 g), followed by water (2mL). The mixture was gently shaken until homogeneous, and then ethanol (7.5 mL)was added. Finally, sodium hydroxide (10%, 1.5 mL) was added and the mixture wasgently stirred to ensure complete mixing.Benzaldehyde (3.8 mL) was then added at room temperature in one portion with gentlestirring. The pH of the resulting reaction mixture was determined and adjusted to >10by dropwise addition of 10% sodium hydroxide.Which of the following accurately corresponds to the composition of the precipitate obtained from a mixture of proteins A and B (properties below) by employing the specified (NH4)2SO4 concentration assuming the salt is added in bulk i.e. one step? Protein % (NH4)2SO4 to precipitate A 40 B 70 a. At 30% (NH4)2SO4 : A b. At 40% (NH4)2SO4 : B c. At 60% (NH4)2SO4 : A d. At 70% (NH4)2SO4 : B e. None of the above
- Dissolved 0.273 grams of pure sodium oxalate (Na2C204) in distilled water and added sulfuric acid and titration the solution at 70 °C by using 42.68 ml of KMNO4 solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H2 C204) with 0.1024 N. Calculate the normlity of KMNO4. Note that the molecular weight of sodium oxalate (Na2C204) = 134 and its equivalent weight = 67 * %3DQ1. Dissolved 0.273 grams of pure sodium oxalate (Na2C0.) In distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMnO, solution and has exceeded end point limits by using 1.46 ml of oxalic acid (H , C, 0.) With 0.1024 N. Calculate the normlity of KMnO .. Note that the molecular weight of sodium oxalate (Na, C, 0.) = 134 and its equivalent weight = 67What is/are the principle/s involved on ACIDIMETRIC ASSAY BY DOUBLE INDICATOR TITRATION?
- Dissolved 0.273 grams of pure sodium oxalate (Na2C204) in distilled water and added sulfuric acid and titration the solution at 70 ' C by using 42.68 ml of KMn04 solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (H2 C204) with 0.1024 N. Calculate the normlity of KMn04. Note that the molecular weight of sodium oxalate (Na2C204) 134 and its equivalent weight ; 67 *Is a Kd value of 10.16 reasonable for the extraction of benzoic Acid between methylene chloride and water? Please explain using extraction theory.An impure sample containing carbonate and sodium bicarbonate, weighing 0.5 g, was taken. It was dissolved in distilled water and then flushed with 0.1 N hydrochloric acid. If the burette reading at the end point of the phenolphthalein index is 10.5 milliliters, and at the orange methyl index end point it is equal to 30.1 milliliters. So, the percentage of sodium bicarbonate in the sample is ............., knowing that the molecular weight of sodium bicarbonate is 84 g/mol.