Sort by: What is the order of the reaction with respect to I-? This indicates that H2O2 undergoes oxidation and reduction; more specifically, the oxygen element in H2O2 is the specie that is reduced in H2O and oxidized into O2. seven years later, the us government returned his passport, and du bois left the united states. Answered: 2) Hydrogen peroxide (H2O2) reacts with | bartleby \[6E_\textrm{eq}=E^o_\mathrm{\large Fe^{3+}/Fe^{2+}}+5E^o_\mathrm{\large MnO_4^-/Mn^{2+}}-0.05916\log\mathrm{\dfrac{5[\ce{MnO_4^-}][Mn^{2+}]}{5[Mn^{2+}][\ce{MnO_4^-}][H^+]^8}}\], \[E_\textrm{eq}=\dfrac{E^o_\mathrm{\large Fe^{3+}/Fe^{2+}} + 5E^o_\mathrm{\large MnO_4^-/Mn^{2+}}}{6}-\dfrac{0.05916}{6}\log\dfrac{1}{[\textrm H^+]^8}\], \[E_\textrm{eq}=\dfrac{E^o_\mathrm{\large Fe^{3+}/Fe^{2+}}+5E^o_\mathrm{\large MnO_4^-/Mn^{2+}}}{6}+\dfrac{0.05916\times8}{6}\log[\textrm H^+]\], \[E_\textrm{eq}=\dfrac{E^o_\mathrm{\large Fe^{3+}/Fe^{2+}}+5E^o_\mathrm{\large MnO_4^-/Mn^{2+}}}{6}-0.07888\textrm{pH}\], Our equation for the equivalence point has two terms. A 6.0 x 10-3 mol/(L-5) B 4.0 x 103 mol/(L.) 6.0 x 10-4 mol/(Ls) D 4.0 x 10-4 mol/(Los). The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask. A solution of MnO4 is intensely purple. In this section we demonstrate a simple method for sketching a redox titration curve. The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the stoichiometry shown above. Excess H2O2 is destroyed by briefly boiling the solution. To evaluate a redox titration we need to know the shape of its titration curve. Adding a heterogeneous catalyst to the reaction system. 5 HO(aq) + 2 MnO(aq) + 6 H(aq) 2 Mn(aq) + 8 HO(l) + 5 O(g). During the titration the analyte is oxidized from Fe2+ to Fe3+, and the titrant is reduced from Cr2O72 to Cr3+. Which statements are correct about calculating LaToya s mechanical advantage? The output force is 450 N.E. A further discussion of potentiometry is found in Chapter 11. What was the rate of disappearance of MnO4- at the same time. du bois: social justice leader best supports the theme that a person can make a difference in the world by standing up for justice and equality? The reduction half-reaction for I2 is, \[\textrm I_2(aq) + 2e^-\rightleftharpoons 2\textrm I^-(aq)\], Because iodine is not very soluble in water, solutions are prepared by adding an excess of I. What is most likely the author's intent by mentioning the "Rodeo Drive shopping spree. If the interferent is a reducing agent, it reduces back to I some of the I3 produced by the reaction between the total chlorine residual and iodide. The I3 is then determined by titrating with S2O32 using starch as an indicator. Step 3: Calculate the potential after the equivalence point by determining the concentrations of the titrants oxidized and reduced forms, and using the Nernst equation for the titrants reduction half-reaction. The Journal of Physical Chemistry A 2016, 120 (27) , 5220-5229. https://doi.org/10.1021/acs.jpca.6b01039 In an acid-base titration or a complexation titration, the titration curve shows how the concentration of H 3 O + (as pH) or M n+ (as pM) changes as we add titrant. Despite its availability as a primary standard and its ease of preparation, Ce4+ is not as frequently used as MnO4 because it is more expensive. Figure 9.40 Titration curve for the titration of 50.0 mL of 0.100 M Fe2+ with 0.100 M Ce4+. Earlier we noted that the reaction of S2O32 with I3 produces the tetrathionate ion, S4O62. Solutions 17. AP Chemistry Chapter 5 Flashcards | Quizlet The red points correspond to the data in Table 9.15. The first term is a weighted average of the titrands and the titrants standard state potentials, in which the weighting factors are the number of electrons in their respective half-reactions. \[\mathrm{Ce^{4+}}(aq)+\mathrm{Fe^{2+}}(aq)\rightarrow \mathrm{Ce^{3+}}(aq)+\mathrm{Fe^{3+}}(aq)\], \[\mathrm{2Ce^{4+}}(aq)+\mathrm{H_2C_2O_4}(aq)\rightarrow \mathrm{2Ce^{3+}}(aq)+\mathrm{2CO_2}(g)+\mathrm{2H^+}(aq)\]. In an acidbase titration or a complexation titration, the titration curve shows how the concentration of H3O+ (as pH) or Mn+ (as pM) changes as we add titrant. Solved Given equation: 2 MnO4- + 5 H2O2 + 6 H+ ? 2 Mn2+ + 8 - Chegg NO2(g) is consumed at a faster rate at temperature 2 because more molecules possess energies at or above the minimum energy required for a collision to lead to a reaction compared to temperature 1. The amount of I3 formed is determined by titrating with S2O32 using starch as an indicator. Figure 9.42 Titration curve for the titration of 50.0 mL of 0.0125 M Sn2+ and 0.0250 M Fe2+ with 0.050 M Ce4+. Because the concentration of pyridine is sufficiently large, I2 and SO2 react with pyridine (py) to form the complexes pyI2 and pySO2. How do I estimate H2O2 concentration? | ResearchGate II. In a titration experiment, H2O2(aq) reacts with aqueous - en.ya.guru \[A_\textrm{red}+B_\textrm{ox} \rightleftharpoons B_\textrm{red}+A_\textrm{ox}\]. See Answer If you look back at Figure 9.7 and Figure 9.28, you will see that the inflection point is in the middle of this steep rise in the titration curve, which makes it relatively easy to find the equivalence point when you sketch these titration curves. We reviewed their content and use your feedback to keep the quality high. LaToyauses 50 newtons (N) of force to pull a 500 N cart. The decomposition is characterized by the stoichiometric reaction 1. If this reaction is broken down into reduction and oxidation halves. III. &=\dfrac{\textrm{(0.100 M)(50.0 mL)}}{\textrm{50.0 mL + 60.0 mL}}=4.55\times10^{-3}\textrm{ M} for which value of kkk are there infinitely many (w, z)(w,z)left parenthesis, w, comma, z, right parenthesis solutions? 3.13: Titrations. Orientation of reactant particles during collisions. A man pushes a shopping cart up a ramp. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. (Note: At the end point of the titration, the solution is a pale pink color.) When using MnO4 as a titrant, the titrands solution remains colorless until the equivalence point. Because the total chlorine residual consists of six different species, a titration with I does not have a single, well-defined equivalence point. TiO2+(aq) + 2H+(aq) + e Ti3+(aq) + H2O(l), MoO22+(aq) + 4H+(aq) + 3e Mo3+(aq) + 2H2O(l), VO2+(aq) + 2H+(aq) + e VO2+(aq) + H2O(l), VO2+(aq) + 4H+(aq) + 3e V2+(aq) + 2H2O(l), Several reagents are commonly used as auxiliary oxidizing agents, including ammonium peroxydisulfate, (NH4)2S2O8, and hydrogen peroxide, H2O2. 2. If a redox titration is to be used in a quantitative analysis, the titrand must initially be present in a single oxidation state. Even though iodine is present as I3 instead of I2, the number of electrons in the reduction half-reaction is unaffected. Other redox indicators soon followed, increasing the applicability of redox titrimetry. (Note: At the end point of the titration, the solution is a pale pink color.) when the concentration of Fe2+ is 10 smaller than that of Fe3+. Oxidation-reduction, because H2(g)H2(g) is oxidized. C2H4(gas) + H2 (gas) react to form C2H6 (gas). Experiment 14 Redox titration of potassium permanganate 3 to lower the electric potential between Mn(II) and Mn(VII) ions, thereby inhibiting . \end{align}\], \[\begin{align} Lets use the titration of 50.0 mL of 0.100 M Fe2+ with 0.100 M Ce4+ in a matrix of 1 M HClO4. Our goal is to sketch the titration curve quickly, using as few calculations as possible. We used a similar approach when sketching the complexation titration curve for the titration of Mg2+ with EDTA. Several forms of bacteria are able to metabolize thiosulfate, which also can lead to a change in its concentration. \[E = E^o_\mathrm{\large Fe^{3+}/Fe^{2+}} - \dfrac{RT}{nF}\log\dfrac{[\mathrm{Fe^{2+}}]}{[\mathrm{Fe^{3+}}]}=+0.767\textrm V - 0.05916\log\dfrac{[\mathrm{Fe^{2+}}]}{[\mathrm{Fe^{3+}}]}\tag{9.16}\], For example, the concentrations of Fe2+ and Fe3+ after adding 10.0 mL of titrant are, \[\begin{align} The complexation reaction, \[\textrm I_2(aq)+\textrm I^-(aq)\rightleftharpoons\textrm I_3^-(aq)\]. The oxidation of NO(g) producing NO2(g) is represented by the chemical equation shown above. The volume of titrant is proportional to the free residual chlorine. The titrations end point is signaled when the solution changes from the products yellow color to the brown color of the Karl Fischer reagent. \[\ce{4MnO_4^-}(aq)+\mathrm{2H_2O}(l)\rightleftharpoons\mathrm{4MnO_2}(s)+\mathrm{3O_2}(g)+\mathrm{4OH^-}(aq)\]. Figure 9.42 shows an example of the titration curve for a mixture of Fe2+ and Sn2+ using Ce4+ as the titrant. What was the rate of disappearance of Mn04 at the same time? In 1787, Claude Berthollet introduced a method for the quantitative analysis of chlorine water (a mixture of Cl2, HCl, and HOCl) based on its ability to oxidize indigo, a dye that is colorless in its oxidized state. The potential, therefore, is easier to calculate if we use the Nernst equation for the titrands half-reaction, \[E_\textrm{rxn}= E^o_{A_\mathrm{\Large ox}/A_\mathrm{\Large red}}-\dfrac{RT}{nF}\ln\dfrac{[A_\textrm{red}]}{[A_\textrm{ox}]}\]. There are several common oxidizing titrants, including MnO4, Ce4+, Cr2O72, and I3. When added to a sample containing water, I2 is reduced to I and SO2 is oxidized to SO3. How could the microbes be easily removed from the electrodes for analysis? If 87.5 percent of sample of pure 13th I decays in 24 days, what is the half- life of 131 I? (b) Titrating with Na2S2O3 converts I3 to I with the solution fading to a pale yellow color as we approach the end point. The initial partial pressures of A2 and B2 used in experiment 1 were twice the initial pressures used in experiment 2. The oxygen element in H2O2 is the specie that is reduced in H2O and oxidized into O2. Under these alkaline conditions the dissolved oxygen oxidizes Mn2+ to MnO2. Although thiosulfate is one of the few reducing titrants that is not readily oxidized by contact with air, it is subject to a slow decomposition to bisulfite and elemental sulfur. The simplest experimental design for a potentiometric titration consists of a Pt indicator electrode whose potential is governed by the titrands or titrants redox half-reaction, and a reference electrode that has a fixed potential. In the Jones reductor the column is filled with amalgamated zinc, Zn(Hg), prepared by briefly placing Zn granules in a solution of HgCl2. After each addition of titrant the reaction between the titrand and the titrant reaches a state of equilibrium. liberates a stoichiometric amount of I3. In a titration experiment, H2O2 (aq) reacts with aqueous MnO4- (aq) as represented by the equation above. The amount of I3 produced is then determined by a back titration using thiosulfate, S2O32, as a reducing titrant. Based on a kinetics study of the reaction represented by the equation above, the following mechanism for the reaction is proposed in response, du bois formed the niagara movement in 1905 with several other civil rights leaders. 2I + 2H + + H2O2 I2 + 2H2O If the solution is relatively acidic (with a pH is less than about 3) the rate of reaction 1 is independent of the pH. If the titration reactions stoichiometry is not 1:1, then the equivalence point is closer to the top or to bottom of the titration curves sharp rise. The earliest Redox titration took advantage of the oxidizing power of chlorine. (Note: At the endpoint of the titration, the solution is a pale pink color. The rate of a certain chemical reaction between substances M and N obeys the rate law above. The concentration of unreacted titrant, however, is very small. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2 (aq) in an Erlenmeyer flask. [\textrm{Fe}^{2+}]&=\dfrac{\textrm{initial moles Fe}^{2+} - \textrm{moles Ce}^{4+}\textrm{ added}}{\textrm{total volume}}=\dfrac{M_\textrm{Fe}V_\textrm{Fe} - M_\textrm{Ce}V_\textrm{Ce}}{V_\textrm{Fe}+V_\textrm{Ce}}\\ An interferent that is an oxidizing agent converts additional I to I3. (Note: At the endpoint of the titration, the solution is a pale pink color.) Chemical Reactions 12. Microbes such as bacteria have small positive charges when in solution. An alternative method for using an auxiliary reducing agent is to immobilize it in a column. Additional results for this titration curve are shown in Table 9.15 and Figure 9.36. A 10.00-mL sample is taken and the ethanol is removed by distillation and collected in 50.00 mL of an acidified solution of 0.0200 M K2Cr2O7. du bois rejected this view. When C2H4(g) reacts with H2(g), the compound C2H6(g) is produced, as represented by the equation above. when the khp solution was titrated with naoh, 14.8 ml was required to reach the phenolphthalien end point. Add 1 mL of a starch indicator solution and continue titrating until the blue color of the starchI3 complex disappears (Figure 9.41). This is an indirect analysis because the chlorine-containing species do not react with the titrant. From the reactions stoichiometry we know that, \[\textrm{moles Fe}^{2+}=\textrm{moles Ce}^{4+}\], \[M_\textrm{Fe}\times V_\textrm{Fe} = M_\textrm{Ce}\times V_\textrm{Ce}\], Solving for the volume of Ce4+ gives the equivalence point volume as, \[V_\textrm{eq} = V_\textrm{Ce} = \dfrac{M_\textrm{Fe}V_\textrm{Fe}}{M_\textrm{Ce}}=\dfrac{\textrm{(0.100 M)(50.0 mL)}}{\textrm{(0.100 M)}}=\textrm{50.0 mL}\]. The reaction between potassium permanganate and hydrogen peroxide Because no attempt is made to correct for organic matter that can not be decomposed biologically, or for slow decomposition kinetics, the COD always overestimates a samples true oxygen demand. ELECTROCHEMISTRY APCHEM STUDY GUIDE Flashcards | Quizlet Examples of species contributing to the free chlorine residual include Cl2, HOCl and OCl. The ladder diagram defines potentials where Inred and Inox are the predominate species. 1. The reaction of 15 moles carbon with 30 moles O2. The sample is placed at the top of the column and moves through the column under the influence of gravity or vacuum suction. is reduced to I and S2O32 is oxidized to S4O62. Another example of a specific indicator is thiocyanate, SCN, which forms a soluble red-colored complex of Fe(SCN)2+ with Fe3+. The titration reaction is, \[\textrm{Sn}^{2+}(aq)+\textrm{Tl}^{3+}(aq)\rightarrow\textrm{Sn}^{4+}(aq)+\textrm{Tl}^+(aq)\]. It is observed that, of the reactants above, Oxidation number of Mn changes from +7 In MnO4- to +2 In Mn2+ (evidently reduction), The Oxygen in MnO4- doesn't change oxidation numbers as its oxidation number stays at -2, Oxidation number of Oxygen changes from -1 in H2O2 to -2 In H2O and 0 in O2. In an acidic solution, however, permanganates reduced form, Mn2+, is nearly colorless. Experts are tested by Chegg as specialists in their subject area. So 29.2 gm reacts = 480 29.2/267= 52.6 gm, Calcium (Ca)(On the periodic table, ionization energy increases as you go up and to the right of the periodic table). Two common reduction columns are used. Some indicators form a colored compound with a specific oxidized or reduced form of the titrant or the titrand. The table above shows the data collected. The diagrams above represent solutes present in two different dilute aqueous solutions before they were mixed. The input force is 500 N.D. The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L. Answer: b. Fiona is correct because the diagram shows two individual simple machines. After dissolving the sample in HCl, the iron was brought into the +2 oxidation state using a Jones reductor. The output force is 50 N.C. Because a titrant in a reduced state is susceptible to air oxidation, most redox titrations use an oxidizing agent as the titrant. (Note: At the end point of the titration, the This problem has been solved! It can be noted that even some glycoproteins and nucleic acids give positive results for this test (since they tend to undergo hydrolysis when exposed to strong mineral acids and form monosaccharides). a. Step 1: HBr(g) + O2(g)-- HO2Br(g) slow Subtracting the moles of I3 reacting with Na2S2O3 from the total moles of I3 gives the moles reacting with ascorbic acid. In a titration experiment, H2O2 (aq) reacts with aqueous MnO4- (aq) as represented by the equation above. calculate the How many grams of iron can be made with 21.5g of Fe2O3. \[\ce{IO_4^-}(aq)+3\mathrm I^-(aq)+\mathrm{H_2O}(l)\rightarrow \ce{IO_3^-}(aq)+\textrm I_3^-(aq)+\mathrm{2OH^-}(aq)\]. A conservation of electrons, therefore, requires that each mole of OCl produces one mole of I3. Step 2: NO3(g) + CO (g) -- NO2(g) + CO2g) fast 2MnO4-(aq) +5 H2O2 (aq) + 6H+(aq) -> 5 O2(g) + 2 (Mn2+(aq - Jiskha In a titration experiment, H2O2(aq) reacts with aqueous MnO4^1- (aq) as represented by the equation below. A conservation of electrons for the titration, therefore, requires that each mole of K2Cr2O7 reacts with six moles of Fe2+. The most important class of indicators are substances that do not participate in the redox titration, but whose oxidized and reduced forms differ in color. Oxidizing Fe2+ to Fe3+ requires only a single electron. \end{align}\], \[\begin{align} Atomic Structure 5. The reaction between these two solutions is represented by the balanced equation you provided: 5 H2O2 (aq) + 2 MnO4 - (aq) + 6 H+ (aq) 2 Mn 2+ (aq) + 8 H2O (l) + 5 O2 (g) The metal, as a coiled wire or powder, is added to the sample where it reduces the titrand. Why does the procedure rely on an indirect analysis instead of directly titrating the chlorine-containing species using KI as a titrant? A: In a titration experiment , H2O2(aq) reacts with aqueous MnO4- as represented by the equation- 5 question_answer Q: Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a A quantitative analysis for ethanol, C2H6O, can be accomplished by a redox back titration. A samples COD is determined by refluxing it in the presence of excess K2Cr2O7, which serves as the oxidizing agent. Particle representations of the mixing of Mg(s) and HCl(aq) in the two reaction vessels are shown in figure 1 and figure 2 above. After the equivalence point, however, unreacted indigo imparts a permanent color to the solution. Unit 5 Questions Flashcards | Quizlet Alternatively, we can titrate it using a reducing titrant. Fiona is correct because the diagram shows two individual simple machines. For example, the presence of H+ reminds us that the reactionfs feasibility is pH-dependent.). NO2(g) + CO(g) -NO(g) + CO2g) In oxidizing ascorbic acid to dehydroascorbic acid, the oxidation state of carbon changes from + in C6H8O6 to +1 in C6H6O6. In 1 M HClO4, the formal potential for the reduction of Fe3+ to Fe2+ is +0.767 V, and the formal potential for the reduction of Ce4+ to Ce3+ is +1.70 V. Because the equilibrium constant for reaction 9.15 is very largeit is approximately 6 1015we may assume that the analyte and titrant react completely. The equivalence point is the point at which titrant has been added in exactly the right quantity to react stoichiometrically with the . If you choose from the following M&M colors, 5 green, 6 yellow, 8 blue, and 7 brown, what is the probability for each of the following events? Finally, because each mole of OCl produces one mole of I3, and each mole of I3 reacts with two moles of S2O32, we know that every mole of NaOCl in the sample ultimately results in the consumption of two moles of Na2S2O3. In a titration experiment, H2O2 (aq) reacts with aqueous MnO4- (aq) as represented by the equation above. A 25-mL portion of the diluted sample was transferred by pipet into an Erlenmeyer flask containing an excess of KI, reducing the OCl to Cl, and producing I3. Both the titrand and the titrant are 1M in HCl. A 5.00-mL sample of filtered orange juice was treated with 50.00 mL of 0.01023 M I3. 9.4: Redox Titrations is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. A redox titrations equivalence point occurs when we react stoichiometrically equivalent amounts of titrand and titrant. The sample is first treated with a solution of MnSO4, and then with a solution of NaOH and KI. The end point is found by visually examining the titration curve. A positive reaction for Molisch's test is given by almost all carbohydrates (exceptions include tetroses & trioses). in a titration experiment, h2o2(aq) reacts with aqueous mno4-(aq) as Cool and dilute to 500 mL with demineralized water in a measuring cylinder and mix well.. Figure 9.37b shows the second step in our sketch. The reduction of hydrogen peroxide in acidic solution, \[\mathrm{H_2O_2}(aq)+\mathrm{2H^+}(aq)+2e^-\rightarrow\mathrm{2H_2O}(l)\]. 3 Br2(aq) + 6 OH-(aq) 5 Br-(aq) + BrO3-(aq) + 3 H2O(l). a 1.513 g sample of khp (c8h5o4k) is dissolved in 50.0 ml of di water. The tetrathionate ion is actually a dimer consisting of two thiosulfate ions connected through a disulfide (SS) linkage. Although a solution of Cr2O72 is orange and a solution of Cr3+ is green, neither color is intense enough to serve as a useful indicator. The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law: where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. Explain the effect of each type of interferent has on the total chlorine residual. The moles of K2Cr2O7 used in reaching the end point is, \[\mathrm{(0.02153\;M\;K_2Cr_2O_7)\times(0.03692\;L\;K_2Cr_2O_7)=7.949\times10^{-4}\;mol\;K_2Cr_2O_7}\], \[\mathrm{7.949\times10^{-4}\;mol\;K_2Cr_2O_7\times\dfrac{6\;mol\;Fe^{2+}}{mol\;K_2Cr_2O_7}=4.769\times10^{-3}\;mol\;Fe^{2+}}\], Thus, the %w/w Fe2O3 in the sample of ore is, \[\mathrm{4.769\times10^{-3}\;mol\;Fe^{2+}\times\dfrac{1\;mol\;Fe_2O_3}{2\;mol\;Fe^{2+}}\times\dfrac{159.69\;g\;Fe_2O_3}{mol\;Fe_2O_3}=0.3808\;g\;Fe_2O_3}\], \[\mathrm{\dfrac{0.3808\;g\;Fe_2O_3}{0.4891\;g\;sample}\times100=77.86\%\;w/w\;Fe_2O_3}\]. If 5 moles appears in a rate of 1.0x10mol /(Ls), 2 moles will disappear: 2 moles (1.0x10mol /(Ls) / 5 moles) = 4x10 mol / (Ls). \[\textrm I_3^-(aq)+2e^-\rightleftharpoons 3\textrm I^-(aq)\]. Water molecules are not shown. The efficiency of chlorination depends on the form of the chlorinating species. Chad is correct because more than one machine is shown in the diagram. Calculate the %w/v ethanol in the brandy. The redox buffer spans a range of volumes from approximately 10% of the equivalence point volume to approximately 90% of the equivalence point volume. Calculate the titration curve for the titration of 50.0 mL of 0.0500 M Sn2+ with 0.100 M Tl3+. Consider, for example, a titration in which a titrand in a reduced state, Ared, reacts with a titrant in an oxidized state, Box. In a typical analysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. You may recall from Chapter 6 that the Nernst equation relates a solutions potential to the concentrations of reactants and products participating in the redox reaction. Although we can easily calculate the potential using the Nernst equation, we can avoid this calculation by making a simple assumption. PDF DETERMINATION OF HYDROGEN PEROXIDE: TITRATION BASED - ResearchGate Methanol is included to prevent the further reaction of pySO3 with water. Report the ores iron content as %w/w Fe2O3.

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