Preparation and Standardization of 0.1 N lodine Solution Preparation 1. Dissolve 14 g of iodine in a solution of 36 g of potassium iodide in 100 ml of water 2. Add 3 drops of hydrochloric acid and dilute to 1000 ml Standardization 1. Weigh 150 mg of arsenic trioxide (As203) and dissolve in 20 ml of 1 N sodium hydroxide by warming it necessary 2. Dilute with 40 ml of water, add 2 drops of methyl orange TS and follow with diluted hydrochloric acid until the yellow color is changed to pink 3. Add 2 grams of sodium bicarbonate, dilute with 50 ml off water, and add 3 ml of starch TS 4. Slowly titrate the lodine solution into the analyte until a permanent blue color is produced. 5. Calculate the normality. "Volume of iodine which produced the permanent blue color: 30.2 ml Standardization: REACTION Arsenic Trioxide Volume of iodine Normality As2O3 + 6NaOH → 2Na3AsO3 + 3H₂O Na3ASO3 + 12 + NaHCO3 → Na3AsO4 + Nal + CO₂ + H₂O DATA 0.150 g 30.2 mL

Preparation and Standardization of 0.1 N lodine Solution Preparation 1. Dissolve 14 g of iodine in a solution of 36 g of potassium iodide in 100 ml of water 2. Add 3 drops of hydrochloric acid and dilute to 1000 ml Standardization 1. Weigh 150 mg of arsenic trioxide (As203) and dissolve in 20 ml of 1 N sodium hydroxide by warming it necessary 2. Dilute with 40 ml of water, add 2 drops of methyl orange TS and follow with diluted hydrochloric acid until the yellow color is changed to pink 3. Add 2 grams of sodium bicarbonate, dilute with 50 ml off water, and add 3 ml of starch TS 4. Slowly titrate the lodine solution into the analyte until a permanent blue color is produced. 5. Calculate the normality. "Volume of iodine which produced the permanent blue color: 30.2 ml Standardization: REACTION Arsenic Trioxide Volume of iodine Normality As2O3 + 6NaOH → 2Na3AsO3 + 3H₂O Na3ASO3 + 12 + NaHCO3 → Na3AsO4 + Nal + CO₂ + H₂O DATA 0.150 g 30.2 mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the Ksp of a compound MX with a solubility of 3.85 × 10–4 g/L, and a molar mass of 146 g/mol. This is a fake compound; M represents some metal and X represents the anion in this ionic compound. Your answer must be consistent with the information given in this problem. Enter your answer in scientific notation, with two decimal places. Example: 1.22e-5 NOTE you must use the letter e and NOT 10.
solution of 1.00 M HCL? 10) How can you prepare 500 ml of 0.1M HCI, if the percentage is 35%, and density = 1.18g/ml, M.mass=36.5 g/mol %3D
What is the volume needed for dH2O
3. Which solution has the highest molarity? Show all the calculations and explain your answer: a) 240g of MgSO4 in 3.0L H₂O 486.5g of Pb(NO3)2 in 0.75L H₂O b) c) 138.0g of CH3CH₂OH in 3.0L H₂O d) 174g of NaCl in 2.0L H₂O e) 85.0g of NaNO3 in 2.0L H₂O
12. The Environmental Protection Agency limit for nitrates in drinking water samples is 10.0 ppm (1.00 ppm = 1.00 × 10° kg/L). The concentration of nitrates in Morro Bay Estuary was measured this morning at 0.6411 mg/L. Does this meet EPA standards? Show your calculations and explain. -6 Name
Calculate the final concentration when a 28.0 mL sample of 25% (m/v) sodium chloride solution is diluted to 250 mL?
What is the solubility of hydrochloric acid at 60 degrees of Celsius? Solubility Curves 150 140 KI 130 120 NANO, KNO, 110 100 90 80 HC NH.CI 70 60 NH, 50 40 NaCI 30 KCIO, 20 10 SO, 10 20 30 40 50 60 70 80 90 100 Temperature °C Grams of solute/100 g H,O 身

Q68 Kindly solve this question in 20 minutes and get the thumbs up Please show me neat and clean work for it By hand solution needed
Chemistry Question
3. Suppose that a 10M of NaCl solution with a volume of 3000ml is heated and looses 1.5liters of its water content. What would be the final concentration of your NaCl sample? MW- Na:23, CI:35
Need help, please.
Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…