Titration of the I2 (254 g/mol) produced from 0.1142 g of primary-standard KIO3 (214 g/mol) required 27.95 mL of Na2S2O3. The concentration of the Na2S2O3 (158 g/mol) solution is ___________
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Titration of the I2 (254 g/mol) produced from 0.1142 g of primary-standard KIO3 (214 g/mol) required 27.95 mL of Na2S2O3. The concentration of the Na2S2O3 (158 g/mol) solution is ___________
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- Pls do fast and i will rate instantly for sure Solution must be in typed form A 25.0 mL volume of 0.0106 M KIO3 is pipetted into a 250-mL Erlenmeyer flask. The solution is titrated to the stoichiometric point with 16.25 mL of a sodium thiosulfate solution. What is the molar concentration of the sodium thiosulfate solution?Molarity of (NH3) solution (M) from bottle- 5.0 Initial reading of buret (NH3) (mL)- .27 Final reading of buret (NH3) (mL)- 8.25 Volume of Cd(NO3)2 solution (mL)- 10.00 Volume of Na2C2O4 solution (mL)- 10,00 please find Total volume of solution after titration (mL) Total moles of C2O42- (mol) Molarity of C2O42- (M) Total moles of Cd2+ (mol) Moles of [Cd(NH3)4]2+ (mol) Molarity of [Cd(NH3)4]2+ (M) Moles of NH3 added by titration (mol) Moles of NH3 that did not react with Cd2+ (mol) Molarity of NH3 that did not react with Cd2+ (M) Kf for [Cd(NH3)4]2+A sodium thiosulfate solution is standardized using pure copper as the primary standard. A sample of copper weighing 0.2624 g is dissolved in acid, excess KI is added, and the liberated iodine was titrated with 42.18 mL of sodium thiosulfate solution. Calculate the molarity of sodium thiosulfate solution. 2Cu2+ + 4I- → 2CuI + I2 I2 + 2S2O32- → 2I- + S4O62-
- A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?A sample weighing 10.91 g containing an unknown amount of H3PO4 was diluted with water and titrated with a standardized concentration of 0.7255 M NaOH. The endpoint was reached after 27.03 mL of the titrant was added. What is the % H3PO4 (97.994 g/mole) in the sample? H3PO4 + 2 NaOH --> Na2HPO4 + 2H2O ROUND OFF FINAL ANSWER TO FOUR (4) SIG FIGS1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.
- Suppose that you use 0.75 g of iron in this experiment. What is the minimum volume of 1.5 M CuSO4 solution required a) using eq. (5-1)? Fe(s) + Cu2+(aq) -> Fe2+(aq) + Cu(s) b) using eq. (5-2)? 2Fe(s) + 3Cu2+(aq) -> 2Fe3+(aq) + 3Cu(s)A. Why is the titration of the oxalate in the green salt with KMnO4 performed prior to carrying out the redox titration for iron content? (Why can’t you do them the other way – iron first then oxalate?) B. In a titration using 0.02000 M KMnO4 solution, the following data were obtained: Buret readings: FINAL = 15.31 mL INITIAL = 5.02 mL How many moles of KMnO4 were used?A 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
- 3. You perform an alkalinity test on a water sample with an initial pH of 9.75. The alkalinity is 12.1mg/L as CaCO3.(a) Calculate the CT value. Answer: 1.54×10-4 M(b) Determine whether there is any potential to precipitate CaCO3 in the pipes given a calciumconcentration of 15 mg/L. Justify your answer. Answer: Calculations show that it exceeds the Ksp, so yesthere is a potential.(c) For the same calcium concentration and CT, determine the potential to precipitate CaCO3 if the pHwere to be lowered to 7. Answer: No, but why? Show calculations to support your answer.A redox titration requires 30.65 mL of iodine solution to titrate a sample containing 25.00 mL of 0.0002487 M ascorbic acid to the end point. What is the molarity of the iodine? options: 0.0002029 M 0.2487 M 0.3049 M 0.0003049 M 0.0002487 M 0.2029 MYou want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an EDTA back titration. CaCO3 has a Ksp of 5x10-9. You add 50.00 mL of 0.3484 M CaCl2 to 500.0ml of sample and filter the solution to remove the precipitate. You then take 250.0 mL of the filtered solution and titrate with 0.1786 M EDTA. You require 23.72 mL to reach the endpoint. What is the concentration of carbonate in the original sample?