A 25.00 mL of pond water was analyzed using Winkler method. A standardized sodium thiosulfate (0.1000 M) was used to titrate the water sample. a. Calculate the moles of sodium thiosulfate reacted to the sample if 1.75 mL was used during the titration. b. How much moles of I2 reacted with the manganese oxide precipitate?
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A 25.00 mL of pond water was analyzed using Winkler method. A standardized sodium thiosulfate (0.1000 M) was used to titrate the water sample.
a. Calculate the moles of sodium thiosulfate reacted to the sample if 1.75 mL was used during the titration.
b. How much moles of I2 reacted with the manganese oxide precipitate?
c. Compute for the dissolved oxygen in the sample. Express the concentration in ppm.
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- 3. It is used to convert the known weight of the precipitate to the corresponding weight of the analyte. a. Gravimetric factor b. Mole ratio c. Mass ratio d. All of the choices 4. Which of the following is used to express the ppm of the solution? a. Kg analyte/liter solution b. Mg analyte/liter solution x 10^6 G analyte/ g sample x 10^6 d. Kg analyte/kg sample C.17. This type of analysis implies that the constituent determined was present in very, very low concentration. a. Macro analysis b. Semi-macro analysis c. Micro analysis 18. Which of the following does not happen during digestion? The crystals dissolve and re-precipitate under equilibrium conditions. b. Weakly bound water are lost from the precipitates. c. Filterability improves d. None of the choicesIs prepared by dissolving a definite weight of a substance in a definite volume. a. primary standard b. secondary standard c. standard addition d. standard sample e. standard solution
- 1. Which among these is/are desirable properties for the type of precipitate required in gravimetric analysis? I. large particles III. known composition A. I only II. reactive with atmospheric constituents IV. small particles C. I & III В. I & II D. III & IV Е. I, П, Ia. What is the concentration of the titrant in Normality? b. What is the mEq of KOH in mg/gram? c. Find the acid value of the sample d. Find the saponification Value of the sample...Which is correct about the prereduction or preoxidation reagents a. Convert the titrant into desired form b. Totally convert analyte into desired form C. Should form a soluble product when react with analyte d. Be difficult to remove from the reaction mixture
- Following the monograph procedure, a 724-mg of aspirin (MW=180 g/mol) dissolved in 18.5 ml of cold neutralized alcohol. This solution was then initially titrated with 0.101 N sodium hydroxide solution, then later neutralized with 0.104 sulfuric acid. 1. What is the total volume (mL) of excess titrant used in the titration? a. 56.400 mL b. 52.000 mL c. 44.600 mL 2. What is the milliequivalent weight consumed by the acidic titrant? a. 1.5392 g-meq b. 2.0907 g-meq c. 1.4948 g-meq d. 2.1528 g-meq 3. What is the milliequivalent weight consumed by the basic titrant? a. 5.8656 g-meq b. 1.5392 g-meq c. 5.6964 g-meq d. 1.4948 g-meq 4. What is the difference of milliequivalent weight consumed in the reaction? a. -4.1572 g-meq b. 4.3708 g-meq c. 0.5515 g-meq d. 4.1572 g-meq 5. What is the percentage purity of the sample? 6. What is the titer value (mg) based from the specific type of titration?Preparation of HCI solution a. Measure 20.7 ml of concentrated Hcl (37% wt HCI) using the pipet and transfer into a 250 ml volumetric flask containing 50 ml of CO2-free distilled water. b. Swrl the solution and dilute with CO2-free distilled water up the mark c. Shake the solution A. d. Calculate the concentration of the HCI 4. Preparation of NaOH solution a. Measure 10g of solid reagent grade NaOH pellets using the analytical balance b. Dissolve the NAOH pellets in 100mL of CO2-free distilled water in a beaker c. Transfer the solution into a 250 ml volumetric flask and dilute to the mark d. Shake the solution e. Calculate the concentration of the NaOH SolutionIvan B. Garcia A. What is the acid/base ratio? Why is it important in the titrimetric process? B. Why should you boil the sample solution right before reaching the end point? c. Does the primary standard used for the standardization of HCI fit the criteria for a good primary standard? Why or Why not?
- Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-mL mark IV. Prepare a contrast paper to determine burette volume and titration endpoint1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/LA 1.067g sample of magnesium oxide of 84.736% were treated with 50mL of 1.017 N Sulfuric Acid, and a 5.195mL volume of sodium hydroxide is required in the back titration. 1. What is the equivalent weight consumed by the acidic titrant? A. 5.281 g-meq B. 55.150 g-meq C. 5.723 g-meq D. 50.850 g-meq 2. What is the difference of milliequivalent weight consumed in the reaction? A. 45.127g-meq B. 56.573g-meq C. 50.850g-meq D. 55.150g-meq 3. What is the amount (in mg) of the analyte that is equivalent to 1 milliliter of the tirant at its equivalence point? A. 22.060mg B. 40.680mg C. 44.12mg D. 20.340mg