Question

What is the Balanced Chemical Equation? The FAS confuses me. please explain

no 4 permanganate Experiment 30 Oxidation-Reduction Titration and Analysis of an Unknown Mixture PURPOSE OY BXPERIMENT: Standardizo a solution of Kno4, and determine the percent by mass of Na2C204 in an unknown mixture. The process of titration may be used for the standardization of solu- tions of oxidizing and/or reducing agents, provided a suitable method for observing the andpoint of the reaction is available. When potassium peran- ganata, Kinos, is used as a titrant, the endpoint is easily apparent. intensely purple colored MnO4 in acidic solution produces the manganeso(II) The ion, which is very palo pink in color, but dilute solutions are practically colorless. Thus, as MnO4 is initially added to a solution of a reactant, the resulting solution will remain essentially colorless. After colorless excess Mno," has been added, the solution will have a pink color. In this experiment you will prepare a dilute solution of NO and standardize1t by titration with an acidified solution of ferrous amonium sulfate hexahydrate, Fe(NH4)2 (804) 2.6H20. During standardization, noe reacts very rapidly at room temperature with iron (II) in acidic solution to produce solutions of manganese (II) and iron(III). You will then use your standardized solution of MnO4" to analyze a mixture of sodium oxalate, Na2C204, and a second component, potassium sulfate, K2504, which does not react with Mno4. The oxalate lon reacts slowly in dilute acidic solutions with Mno, to produce carbon dioxide and manganeso(II) ion. Since this reaction is slow at room temperature, the solution containing the oxalate ion will be heated and titrated at 55°c. In addition, the rate of reaction will be enhanced by the formation of manganese (II) because manganese (II) is an autocatalyst. In autocatalysis, a product of the reaction acts as a catalyst of the reaction. By knowing the balanced chemical equation and the number of moles of Mno,which react, the number of moles of oxalate ion and The number of the number of moles of sodium oxalate can be calculated. moles of sodium oxalata can, in turn, be used to calculate the percent composition by mass of sodium oxalate in the unknown mixture.

Answer 1

Fe (NH4)2 (soy). (H, O) → Fe2(aq) + 2N Hy Lag) + 25042 Caop) +8H, 011) 5fe2t + MnO4 + 8H7 = 5fe3+ + Moz+(aq) + 4H2011) Molecular wt. of Fe (NH4)₂(SO4)₃ (H₂O = 392. 1 glmol Wt. of Fe (NH4), Bouzky ) = 0.64599 t moles of Fe (Nty). (Souz (H₂O) = 0.64 34 g 392-19. molt = 0.00165 mol -t mole Fe (NH)(Sop), (1, 0)6 = 1 mol fe2f to moles of Fe2+ = 0.00165 md - 5 moles Feet reacts with I mol mnou moles of Mnou = 0.00165 = 0.00033 mol 3) moles of_k Mner used = 0.00033 mol Volume of Km nou used = 27.21-3.24 = 23.97 ml 0.00033 mot Molarity of KMnO4 = 0 0.02397L a 0.014 M