If 0.3800g of KIIO3 (214.00 g/mol) was used to liberate free iodine which was then titrated with 205.80 mL sodium thiosulfate (158.11 g/mol) solution. Calculate the concentration of thiosulfate solution in mg/ml KIO3 + 5KI + 6 HCl ---- 3H20 +312+6KCI 2Na2S203 + 12 Na2S406 + 21
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- A 0.1017-g sample of KBrO3 (MW = 167 g/mole) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated iodine required 39.75 mL of a sodium thiosulfate solution. Calculate the molar concentration of the Na2S2O3. BrO3 - + 6I + 6HCl → Br - + 3I2 + 6KCl + 3H2O I2 + Na2S2O3 → 2NaI + Na2S4O6 The type of redox titration reaction is ___. a. iodimetry b. bromination c. iodometry d. diazotination The role of KBrO3 in the titration is ___. a. reducing agent b. oxidizing agent c. source of Br2 d. source of I2 At the endpoint of titration, the equivalence of sodium thiosulfate is equal to the following, EXCEPT ___ . a. equivalence of KI b. equivalence of liberated I2 c. equivalence of KBrO3 d. none of the other choicesA 0.1017 g sample of KBrO3 (MM=166.1) was dissolved in dilute HCI and treated with an unmeasured excess of Kl. The liberated iodine required 39.75 mL of Na₂S₂O3. Calculate the molar concentration of sodium thiosulfate. 0.2561 M 0.08512 M 0.09242 M 0.1041 MA 0.2500 g sample of swimming pool oxidizer containing calcium hypochlorite as the active ingredient was dissolved in 0.50 M H2SO4 containing KI. The liberated iodine required 38.2 mL of Na2S2O3. The titrant was standardized by titrating 101.3 mg K2Cr2O7 dissolved in acid with the action of excess KI, which required 17.4 mL of the Na2S2O3. Calculate the % Ca(OCl)2 in the sample.
- A 100.0-mL sample of spring water was treated to convert any iron present to Fe2+.Titration with 35.00-mLof 0.002345 M K2Cr2O7 resulted in the reaction6Fe2+ + Cr2O72- + 14H+ 6Fe3+ 1 2Cr3+ + 7H2OThe excess K2Cr2O7 was back-titrated with 8.32 mL of 0.00897 M Fe2+ solution.Calculate the concentration of iron in the sample in parts per million.A solution was prepared by dissolving about 30.00m g of EDTA in approximately 1 L of water and standardizing against 50.00-mL aliquots of 0.004356 M Mg2+. An average titration of 32.65 mL was required. Calculate the molar concentration of the EDTA.An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask. and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, (a) Outline the two steps involved, representing the related reactions. (b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution. (c) Calculate the masses of CaCO3 and MgCO3 present in the pellet. (d) Calculate the…
- . An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, a) Outline the two steps involved, representing the related reactions./5 b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution./6 c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6 d) Calculate…A carbonate fusion ws needed to free the Bi from a 0.6423g sample containing the mineral eulytite (2Bi2O3.3SiO2). The fused mass was dissolved in dilute acid, following which the Bi+3 was titrated with 23.76mL of 0.03369M NaH2PO4. The reaction isBi+3+ H2PO4- ---> BiPO4(s) + 2H+ Calculate the % purity of eulytite (1112g/mol) in the sample. I just do not even know where to begin. I not only need to see steps, but I need good explanation of why the steps were taken. Thanks!A 5.186 gram sample of the anti-malarial pesticide DDT was dissolved in 100.0 mL of alchohol and 10.00 mL aliquots were taken for analysis. One such aliquot was decomposed with metallic sodium, and the liberated chloride ion was precipitated as AgCl. Express the results of this analysis in terms of %DDT (C14H9Cl5, FW = 354.49) based on the recovery of 150 mg of AgCl (FW = 143.32).
- 0.8153 g of a sample containing Pb(NO3)2 was taken, dissolved in water, and 40.20 mL of 0.06 M EDTA was added. If the excess EDTA was back-titrated with 23.10 mL of 0.02 M EDTA, which of the following is the percentage of Pb(NO3)2? (Pb(NO3)2: 331 g/mol, Pb: 207 g/mol) A. 85,23B. 38.25C. 35.63D. 79.17*SHOW COMPLETE SOLUTION* A 4.971g sample containing the mineral tellurite was dissolved and then treated with 50.00mL of 0.03114M K2Cr2O7: 3TeO2 + Cr2O7-2 + 8H+ → 3H2TeO4 + 2Cr+3 + H2O When the reaction is complete, the excess Cr2O7-2 required a 10.05mL back-titration with 0.1135M Fe2+. Calculate the percentage of TeO2 (MM 159.6) in the sample. 6Fe+2 + Cr2O7-2 + 14H+ → 6Fe+3 + 2Cr+3 + 7H2O Answer: 13.17% TeO2A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.