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- To calculate the unknown concentration of a chemical in a solid sample, 4 different calibrationcurves were plot using 4 different methods. Which of the following method is considered asacceptable? a. Method 4, R? = 0.998b. Method 1, R2 = 0.650c. Method 2. R' = 0.890d. Method 3, R' = 0.169 Time remaining: 00 :09 :31 Chemistry DETERMINATION OF BIOLOGICAL OXYGEN DEMAND USING THE MODIFIED WINKLER METHOD GUIDE QUESTIONS: 1. What are the pertinent chemical equations in the standardization of sodium thiosulfate solution? 2. Explain the reason for the addition of H2SO4 and excess KI. 3. What is the effect of adding the acid before KI? 4. Present the pertinent chemical equations involved in the analysis. 5. Explain the stepwise production of titratable 12 from dissolved Oz in the sample. 6. Explain why the reagents are added in the specific sequence described in the experiment. 7. Explain the would-be effects (if any) of the following considerations: a. Water sample was made to stand overnight before analysis b. MnSO4 was added and the solution was made to stand overnight before the analysis 8. What are the possible sources of errors and their effect on the calculated parameters?3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)
- 6. Why do we need to precipitate from a hot solution? 7. Why is the precipitating agent added all at once? 8. What is the purpose of adding 6M HCI in the sample solution? 9. Why do we need to test the washings with AgNO3? 10. What is done in an ignition process? 11. What is the product after the precipitate was ignited? 12. What are the advantages of performing ignition? 13. Cite the sources of errors for this experiment and explain how to possibly circumvent these kinds of problems.A fermenter was filled with 10L of 0.6 mol/L sodium sulfite solution containing 0.003M Cu2+ ion and the air sparger was turned on. After exactly 10 minutes, the airflow was stopped and a 5 mL sample was taken and titrated. The concentration of sodium sulfite in the sample was found to be 0.2 M. Calculate the oxygen uptakeWhat is the ratio of the moles of sodium hydroxide to the moles of crystal violet (nNaOH/nCV+) at the start of the reaction? Make sure to account for the fact that different volumes of the stock solutions are mixed. 5.0 mL 2.0 × 10–5 M crystal violet solution 1.0 mL of 0.10 M NaOH solution Trail. [Na+]j (M) [OH–]j (M) 1 1.67 × 10–2 1.67 × 10–2
- Precipitation of chloride in a sample of a weight of 0.272 g by adding 50 ml of 0.103 N silver nitrate. It is necessary to calibrate the excess amount of 8.65 silver nitrate with 0.126N potassium thiocyanate Calculate the percentage of chloride in the sample?A sodium thiosulfate solution can be standardized by using it to titrate the iodine liberated by the action of excess KI on a known weight of primary standard K2Cr2O7: Cr2O72- + 6I- + 14H+ → 2 Cr3+ + 3I2 + 7H2O I2 + 2S2O32- → 2I- + S4O62- Calculate the molar concentration of the sodium thiosulfate solution if 31.47 mL of this solution were required to titrate a sample prepared using 0.2177 g pure K2Cr2O7.In this experiment you were given the concentration of NaOH(aq). That concentration was determined in part A.1. by using a solid acid, potassium hydrogen phthalate. Suppose the potassium hydrogen phthalate used for the standardization of the sodium hydroxide solution is not completely dry. This technique error will result in the reported concentration of NaOH(aq) to be ____________. a. unaffected b. too high c. too low
- Average mass of the precipitate MgNH4PO4·6H2O (s) / g Average phosphate concentration in water sample (mass/volume %) % difference of 2 trialsA 25.00-mL sample of La31 was treated with excess Na2C2O4 to precipitate La2(C2O4)3, which was washed to remove excess C2O4 22 and then dissolved in acid. The oxalate from La2(C2O4)3 required 12.34 mL of 0.004 321 M KMnO4 to reach the purple end point of Reaction 6-1. Find the molarity of La31 in the unknown.The thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg2+ via the reaction below. Find the percentage of (NH2)2CS (76.12 g/mol) in the sample. 4(NH2)2CS + Hg2+= (NH2)2CS 4Hg2+