If your question is not fully disclosed, then try using the search on the site and find other answers on the subject Chemistry. Both the titrand and the titrant are 1.0 M in HCl. The equivalence point is shown by the red dot. This is an important observation because we can use either half-reaction to monitor the titrations progress. (Note: At the end point of the titration, the solution is a pale pink color. We used a similar approach when sketching the complexation titration curve for the titration of Mg2+ with EDTA. 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. Unit 5 Questions Flashcards | Quizlet The amount of I3 formed is determined by titrating with S2O32 using starch as an indicator. The COD provides a measure of the quantity of oxygen necessary to completely oxidize all the organic matter in a sample to CO2 and H2O. Answered: In carrying out Part 1 of this | bartleby Triiodide also can be used for the analysis of ascorbic acid (vitamin C) by oxidizing the enediol functional group to an alpha diketone. Figure 9.37 Illustrations showing the steps in sketching an approximate titration curve for the titration of 50.0 mL of 0.100 M Fe2+ with 0.100 M Ce4+ in 1 M HClO4: (a) locating the equivalence point volume; (b) plotting two points before the equivalence point; (c) plotting two points after the equivalence point; (d) preliminary approximation of titration curve using straight-lines; (e) final approximation of titration curve using a smooth curve; (f) comparison of approximate titration curve (solid black line) and exact titration curve (dashed red line). The reaction of 15 moles carbon with 30 moles O2. Under the now acidic conditions I is oxidized to I3 by MnO2. Solutions of Ce4+ usually are prepared from the primary standard cerium ammonium nitrate, Ce(NO3)42NH4NO3, in 1 M H2SO4. The change in color from (c) to (d) typically takes 12 drops of titrant. Published in category Chemistry, 11.08.2020 By titrating this I3 with thiosulfate, using starch as a visual indicator, we can determine the concentration of S2O32 in the titrant. Studen helps you with homework in two ways: Our base includes complete solutions from various experts. The input force is 50 N.B. Ethanol is oxidized to acetic acid, C2H4O2, using excess dichromate, Cr2O72, which is reduced to Cr3+. The liberated I3 was determined by titrating with 0.09892 M Na2S2O3, requiring 8.96 mL to reach the starch indicator end point. is added to a solution of ethanoic acid, CH3COOH. First, in reducing OCl to Cl, the oxidation state of chlorine changes from +1 to 1, requiring two electrons. In a titration experiment, H2O2 (aq) reacts with aqueous MnO4- (aq) as represented by the equation above. Even if the total chlorine residual is from a single species, such as HOCl, a direct titration with KI is impractical. The indicator changes color when E is within the range. Which of following rate law is consistent with the proposed mechanism? To determine the stoichiometry between the analyte, NaOCl, and the titrant, Na2S2O3, we need to consider both the reaction between OCl and I, and the titration of I3 with Na2S2O3. Microbes such as bacteria have small positive charges when in solution. 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. In a titration experiment, H2O2 (aq) reacts with aqueous MnO4- (aq) as represented by the equation above. Explain the effect of each type of interferent has on the total chlorine residual. A choice may be used once, more than once, or not at all in each set. Mercuric sulfate, HgSO4, is added to complex any chloride that is present, preventing the precipitation of the Ag+ catalyst as AgCl. H2O2 + I - = H2O + IO - (slow) H2O2 + IO - = H2O + O2 + I - (fast) Which Chemistry (Please check) asked by Hannah 757 views 0 answers The resulting solution is acidified with H 2 SO 4 (aq). Figure 9.37b shows the second step in our sketch. 2AlCl3 + 3Br2 2AlBr3 + 3Cl2, Which of the following will have a lower ionization energy than scandium, Give an example of a protein structure that would give positive test with Molischs Reagent. 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) In 1 M HClO 4, the formal potential for the reduction of Fe 3+ to Fe 2+ is +0.767 V, and the formal potential for the reduction of Ce 4+ to Ce 3+ is +1.70 V. Answers: 5 H2O2 (aq) + 2 MnO4 - (aq) + 6 H+ (aq) 2 Mn 2+ (aq Although each method is unique, the following description of the determination of the total chlorine residual in water provides an instructive example of a typical procedure. Table 9.17 provides a summary of several applications of reduction columns. (Note: At the end point of the titration, the solution is a pale pink color.) PDF Redox titrations with potassium permanganate - At the titrations equivalence point, the potential, Eeq, in equation 9.16 and equation 9.17 are identical. 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). Select the one lettered choice that best fits each statement. During the titration the analyte is oxidized from Fe2+ to Fe3+, and the titrant is reduced from Cr2O72 to Cr3+. Step 1: Calculate the volume of titrant needed to reach the equivalence point. \[E_\textrm{rxn}=E_{B_\mathrm{\Large ox}/B_\mathrm{\Large red}}-E_{A_\mathrm{\Large ox}/A_\mathrm{\Large red}}\]. How many moles of HF are in 30.mL of 0.15MHF(aq) ? Take the blank into account and express the titration result as grams of hydrogen peroxide present in 100 mL of the sample. If the concentration of dissolved O2 falls below a critical value, aerobic bacteria are replaced by anaerobic bacteria, and the oxidation of organic waste produces undesirable gases, such as CH4 and H2S. The following questions refer to the reactions represented below. Covalent Bonding 10. in a titration experiment, h2o2(aq) reacts with aqueous mno4-(aq) as What is the order of the reaction with respect to I-? The Mole 11. \end{align}\], \[\begin{align} Other titrants require a separate indicator. provides the necessary electrons for reducing the titrand. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2 (aq) in an Erlenmeyer flask. The reaction can be balanced by presuming that it occurs through two separate half-reaction. \[\mathrm{Ce^{4+}}(aq)+\mathrm{Fe^{2+}}(aq)\rightarrow \mathrm{Ce^{3+}}(aq)+\mathrm{Fe^{3+}}(aq)\], \[\mathrm{2Ce^{4+}}(aq)+\mathrm{H_2C_2O_4}(aq)\rightarrow \mathrm{2Ce^{3+}}(aq)+\mathrm{2CO_2}(g)+\mathrm{2H^+}(aq)\]. Derive a general equation for the equivalence points potential when titrating Fe2+ with MnO4. Chlorine may be present in a variety of states, including the free residual chlorine, consisting of Cl2, HOCl and OCl, and the combined chlorine residual, consisting of NH2Cl, NHCl2, and NCl3. Methanol is included to prevent the further reaction of pySO3 with water. \[E_\textrm{rxn}= E^o_{B_\mathrm{\Large ox}/B_\mathrm{\Large red}}-\dfrac{RT}{nF}\ln\dfrac{[B_\textrm{red}]}{[B_\textrm{ox}]}\], Lets calculate the titration curve for the titration of 50.0 mL of 0.100 M Fe2+ with 0.100 M Ce4+ in a matrix of 1 M HClO4. Depending on the sample and the method of sample preparation, iron may initially be present in both the +2 and +3 oxidation states. 2 H2O2(aq) 2 H2O(l) + O2(g) H = 196 kJ/molrxn, AP Chem Unit 4.8: Introduction to Acid-Base R, AP Chem Unit 4.9: Oxidation-Reduction (Redox), AP Chemistry | Unit 3 Progress Check: MCQ, AP Chem Unit 6.5: Energy of Phase Changes, AP Chem Unit 6.4: Heat Capacity and Calorimet, AP Chem Unit 6.3: Heat Transfer and Thermal E, Bruce Edward Bursten, Catherine J. Murphy, H. Eugene Lemay, Matthew E. Stoltzfus, Patrick Woodward, Theodore E. Brown. Measurements 4. One of the most important applications of redox titrimetry is evaluating the chlorination of public water supplies. Which titrant is used often depends on how easy it is to oxidize the titrand. Before the equivalence point, the potential is determined by a redox buffer of Fe2+ and Fe3+. Second, in the titration reaction, I3. 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). 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. Solutions of MnO4 are prepared from KMnO4, which is not available as a primary standard. Which of the diagrams below is the best particle representation of the mixture after the precipitation reaction occurred? The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2 (aq) in an Erlenmeyer flask. The initial partial pressures of A2 and B2 used in experiment 1 were twice the initial pressures used in experiment 2. 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, \[\mathrm{4.769\times10^{-3}\;mol\;Fe^{2+}\times\dfrac{1\;mol\;Fe_2O_3}{2\;mol\;Fe^{2+}}\times\dfrac{159.69\;g\;Fe_2O_3}{mol\;Fe_2O_3}=0.3808\;g\;Fe_2O_3}\], \[\mathrm{\dfrac{0.3808\;g\;Fe_2O_3}{0.4891\;g\;sample}\times100=77.86\%\;w/w\;Fe_2O_3}\]. A comparison of our sketch to the exact titration curve (Figure 9.37f) shows that they are in close agreement. is similar to the determination of the total chlorine residual outlined in Representative Method 9.3. 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. Provides a comparison of the initial rate of formation of AB in experiments 1 and 2. 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+. \[\ce{IO_4^-}(aq)+\mathrm{H_2O}(l)+2e^-\rightleftharpoons \ce{IO_3^-}(aq)+\mathrm{2OH^-}(aq)\]. If 87.5 percent of sample of pure 13th I decays in 24 days, what is the half- life of 131 I? An alternative method for using an auxiliary reducing agent is to immobilize it in a column. Earlier we noted that the reaction of S2O32 with I3 produces the tetrathionate ion, S4O62. In the same fashion, I3 can be used to titrate mercaptans of the general formula RSH, forming the dimer RSSR as a product. Legal. Water molecules are not included in the particle representations. When NaHCO3 completely decomposes, it can follow this balanced chemical The titrant can be used to directly titrate the titrand by oxidizing Fe2+ to Fe3+. III. For a back titration we need to determine the stoichiometry between I3 and the analyte, C6H8O6, and between I3 and the titrant, Na2S2O3. Explain why an increase in temperature increases the rate of a chemical reaction. A further discussion of potentiometry is found in Chapter 11. X H2O (s), is heated, H2O (molar mass 18 g) is driven off. See answers Solved Refer to the following types of chemical or physical | Chegg.com 25 Step-by-step answer Microbes in the water collect on one of the electrodes. A metal that is easy to oxidizesuch as Zn, Al, and Agcan serve as an auxiliary reducing agent. (Note: At the end point of the titration, the solution is a pale pink color.) Chad is correct because the diagram shows two simple machines doing a job. Executive support systems are information systems that support the:? Figure 9.42 shows an example of the titration curve for a mixture of Fe2+ and Sn2+ using Ce4+ as the titrant. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask. The oxidation of NO(g) producing NO2(g) is represented by the chemical equation shown above. Question: Question 2 SH2O2(aq) + 2 MnO( +6H -2mnd+8H201 +502) In a titration experiment, Halach reacts with aqueous MnO (adas represented by the equation above. &\mathrm{= \dfrac{(0.100\;M)(50.0\;mL)-(0.100\;M)(10.0\;mL)}{50.0\;mL+10.0\;mL} = 6.67\times10^{-2}\;M} Introduction to Chemistry 2. Oxidation is defined as the outright loss of electrons. Experiment 14 Redox titration of potassium permanganate 3 to lower the electric potential between Mn(II) and Mn(VII) ions, thereby inhibiting . H3AsO4 + 3I- + 2H3O+ -- H3AsO3 + I3- + H2O 2HBr (g) + O2(g) -- H2O2(g) +Br2 (g) As shown in the following two examples, we can easily extend this approach to an analysis that requires an indirect analysis or a back titration. he was against any form of compromise and in favor of full and immediate equality. Instead, adding an excess of KI reduces the titrand, releasing a stoichiometric amount of I3. The purity of a sample of sodium oxalate, Na2C2O4, is determined by titrating with a standard solution of KMnO4. It is clear by the equation 2(27+335.5)= 267 gm of AlCl3 reacts with 6 80 = 480 gm of Br2 . This apparent limitation, however, makes I2 a more selective titrant for the analysis of a strong reducing agent in the presence of a weaker reducing agent. The diagrams above represent solutes present in two different dilute aqueous solutions before they were mixed. Gases in general are ideal when they are at high temperatures and low pressures. seven years later, the us government returned his passport, and du bois left the united states. This reaction is catalyzed by the presence of MnO2, Mn2+, heat, light, and the presence of acids and bases. (Note: At the endpoint of the titration, the solution is a pale pink color.) Each FAS formula unit contains one Fe 2+. For example, NO2 interferes because it can reduce I3 to I under acidic conditions. )Which element is being oxidized during . NO2(g) + CO(g) -NO(g) + CO2g) Diphenylamine sulfonic acid, whose oxidized form is red-violet and reduced form is colorless, gives a very distinct end point signal with Cr2O72. Chad is correct because more than one machine is shown in the diagram. in a titration experiment, h2o2 (aq) reacts with aqueous mno4- (aq) as represented by the equation above. At a pH of 1 (in H2SO4), for example, the equivalence point has a potential of, \[E_\textrm{eq}=\dfrac{0.768+5\times1.51}{6}-0.07888\times1=1.31\textrm{ V}\]. Aqueous solutions of permanganate are thermodynamically unstable due to its ability to oxidize water. An interferent that is an oxidizing agent converts additional I to I3. The output force is 450 N.E. \[\textrm I_3^-(aq)+2e^-\rightleftharpoons 3\textrm I^-(aq)\]. First, we add a ladder diagram for Ce4+, including its buffer range, using its EoCe4+/Ce3+ value of 1.70 V. Next, we add points representing the potential at 110% of Veq (a value of 1.66 V at 55.0 mL) and at 200% of Veq (a value of 1.70 V at 100.0 mL). calculate the How many grams of iron can be made with 21.5g of Fe2O3. The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the stoichiometry shown above. The mechanical advantage is 10.F. Orientation of reactant particles during collisions. In a titration experiment, H2O2 (aq) reacts with aqueous MnO4^1- (aq) as represented by the equation below.The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2 (aq) in anErlenmeyer flask. 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. After the equivalence point, however, unreacted indigo imparts a permanent color to the solution. The first task is to calculate the volume of Ce4+ needed to reach the titrations equivalence point. Because it is difficult to completely remove all traces of organic matter from the reagents, a blank titration must be performed. The amount of I3 formed is then determined by titrating with Na2S2O3 using starch as an indicator. After the oxidation was complete, 13.82 mL of 0.07203 M Na2S2O3 was needed to reach the starch indicator end point. Rate = k[I ]a[H2O2]b Another method for locating a redox titrations end point is a potentiometric titration in which we monitor the change in potential while adding the titrant to the titrand. Under these conditions, the efficiency for oxidizing organic matter is 95100%. Which of the reactions will initially proceed faster and why? 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 oxidized and reduced forms of some titrants, such as MnO4, have different colors. The complexation reaction, \[\textrm I_2(aq)+\textrm I^-(aq)\rightleftharpoons\textrm I_3^-(aq)\]. Two experiments were done at the same temperature inside rigid containers. 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. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask. (please explain it)Options6.0 x 10-3 mol/(Ls)A4.0 x 10-3 mol/(Ls)B6.0 x 10-4 mol/(Ls)C4.0. Because it is a weaker oxidizing agent than MnO4, Ce4+, and Cr2O72, it is useful only when the titrand is a stronger reducing agent. Under the same conditions, one of the following graphs represents the changes in the concentration of O2(g) over the same period of time. Because the equilibrium constant for reaction 9.4.1 is very largeit is approximately 6 1015 we may assume that the analyte and titrant react completely. 1) The decomposition of hydrogen peroxide in solution and in the presence of iodide ion was studied in laboratory, and the following mechanism proposed based on the experimental data. In a titration experiment, H2O2(aq) reacts with aqueous MnO4-(aq) as represented by the equation above. 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. If this reaction is broken down into reduction and oxidation halves. The graph above shows the distribution of energies for NO2(g) molecules at two temperatures. One standard method for determining the dissolved O2 content of natural waters and wastewaters is the Winkler method. The description here is based on Method 4500-Cl B as published in Standard Methods for the Examination of Water and Wastewater, 20th Ed., American Public Health Association: Washington, D. C., 1998. You may recall from Chapter 6 that a redox buffer operates over a range of potentials that extends approximately (0.05916/n) unit on either side of EoFe3+/Fe2+. Iodine has been used as an oxidizing titrant for a number of compounds of pharmaceutical interest. A titrant can serve as its own indicator if its oxidized and reduced forms differ significantly in color. A 25.00-mL sample of a liquid bleach was diluted to 1000 mL in a volumetric flask. When prepared using a reagent grade material, such as Ce(OH)4, the solution is standardized against a primary standard reducing agent such as Na2C2O4 or Fe2+ (prepared using iron wire) using ferroin as an indicator. Next, we add points representing the pH at 10% of the equivalence point volume (a potential of 0.708 V at 5.0 mL) and at 90% of the equivalence point volume (a potential of 0.826 V at 45.0 mL). Figure 9.38 shows a typical titration curve for titration of Fe2+ with MnO4. Oxidation-reduction, because H2(g)H2(g) is oxidized. The oxidized DPD is then back titrated to its colorless form using ferrous ammonium sulfate as the titrant. Figure 9.40 Titration curve for the titration of 50.0 mL of 0.100 M Fe2+ with 0.100 M Ce4+. Select all that apply.A. This problem can be minimized by adding a preservative such as HgI2 to the solution. 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. It takes five moles of Fe 2+ to react with one mole of KMnO 4 according to the balanced chemical equation for the reaction. liberates a stoichiometric amount of I3. As with acidbase titrations, we can extend a redox titration to the analysis of a mixture of analytes if there is a significant difference in their oxidation or reduction potentials. The scale of operations, accuracy, precision, sensitivity, time, and cost of a redox titration are similar to those described earlier in this chapter for acidbase or a complexation titration. In the Walden reductor the column is filled with granular Ag metal. This approach to standardizing solutions of S2O32. The reaction between IO3 and I, \[\textrm{IO}_3^-(aq)+8\textrm I^-(aq)+6\textrm H^+(aq)\rightarrow \ce{3I_3^-}(aq)+\mathrm{3H_2O}(l)\]. 5.1 and 5.5 Practice Flashcards | Quizlet A partial list of redox indicators is shown in Table 9.16. Created by Jay. 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 &=\dfrac{\textrm{(0.100 M)(50.0 mL)}}{\textrm{50.0 mL + 60.0 mL}}=4.55\times10^{-3}\textrm{ M} Water is sent between the two oppositely charged electrodes of a parallelplate capacitor. Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L. An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Excess H2O2 is destroyed by briefly boiling the solution. The table above shows the data collected. In the Jones reductor the column is filled with amalgamated zinc, Zn(Hg), prepared by briefly placing Zn granules in a solution of HgCl2. The mass of a sample of the iron(II) compound is carefully measured before the sample is dissolved in distilled water. Examples of appropriate and inappropriate indicators for the titration of Fe2+ with Ce4+ are shown in Figure 9.40. \[\ce{MnO_4^-}(aq)+\mathrm{5Fe^{2+}}(aq)+\mathrm{8H^+}(aq)\rightarrow \mathrm{Mn^{2+}}(aq)+\mathrm{5Fe^{3+}}(aq)+\mathrm{4H_2O}(l)\], \[\ce{2MnO_4^-}(aq)+\mathrm{5H_2C_2O_4}(aq)+\mathrm{6H^+}(aq)\rightarrow\mathrm{2Mn^{2+}}(aq)+\mathrm{10CO_2}(g)+\mathrm{8H_2O}(l)\], Potassium dichromate is a relatively strong oxidizing agent whose principal advantages are its availability as a primary standard and the long term stability of its solutions. \[\mathrm{C_6H_8O_6}(aq)+\ce{I_3^-}(aq)\rightarrow \mathrm{3I^-}(aq)+\mathrm{C_6H_6O_6}(aq)+\mathrm{2H^+}(aq)\], \[\ce{I_3^-}(aq)+\mathrm{2S_2O_3^{2-}}(aq)\rightarrow \mathrm{S_4O_6^{2-}}(aq)+\mathrm{3I^-}(aq)\]. n= 0.857 moles (where 28 g/mole is the molar mass of N, that is, the amount of mass that the substance contains in one mole.). To evaluate a redox titration we need to know the shape of its titration curve. Subtracting the moles of I3 reacting with Na2S2O3 from the total moles of I3 gives the moles reacting with ascorbic acid. Figure 9.39 Diagram showing the relationship between E and an indicators color. Both the titrand and the titrant are 1M in HCl. 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 redox buffer spans a range of volumes from approximately 10% of the equivalence point volume to approximately 90% of the equivalence point volume. Solved: In a titration experiment, H2O2(aq) reacts with aq Next, we draw our axes, placing the potential, E, on the y-axis and the titrants volume on the x-axis. 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. This is an indirect analysis because the chlorine-containing species do not react with the titrant. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask. Because we have not been provided with the titration reaction, lets use a conservation of electrons to deduce the stoichiometry. 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. Another useful reducing titrant is ferrous ammonium sulfate, Fe(NH4)2(SO4)26H2O, in which iron is present in the +2 oxidation state. Before titrating, we must reduce any Fe3+ to Fe2+. (Note: At the end point of the titration, the This problem has been solved!
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