Experiment 6: Redox Titrations (Iodine Titrations) Calculate the concentration of sodium thiosulfate (158.11 g/mol) solution in g/L. if 0.200g of KIO3 (214.00 g/mol) required 60.0 mL of the thiosulfate solution in the presence of excess of KI and H₂SO₂? KIO, +5KI + 3H₂SO4 -3H₂O + 31₂ +3K₂SO4 2Na₂S₂O3 + 1₂ → Na₂S₂O6 + 21- a) 17.7 g/L b) 22.2/L c) 14.8 g/L d) 29.6 g/L e) 12.7 g/L

Experiment 6: Redox Titrations (Iodine Titrations) Calculate the concentration of sodium thiosulfate (158.11 g/mol) solution in g/L. if 0.200g of KIO3 (214.00 g/mol) required 60.0 mL of the thiosulfate solution in the presence of excess of KI and H₂SO₂? KIO, +5KI + 3H₂SO4 -3H₂O + 31₂ +3K₂SO4 2Na₂S₂O3 + 1₂ → Na₂S₂O6 + 21- a) 17.7 g/L b) 22.2/L c) 14.8 g/L d) 29.6 g/L e) 12.7 g/L

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 37QAP: An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is...

See similar textbooks

Similar questions

An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?
What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?
A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.615 M NaOH. The equivalence point is reached when 33.6 mL are added. What is the unknown acid?
A certain local brand of "healthy" chicharon was found to contain 0.4132 g of NaCl after Fajan titration. How much sodium is present in the sample? MM NaCl-58.44 g/mol; MW Na* = 22.99 g/mol; MW CI=35.45 g/mol Cr + Ag+ AgCl(s) O 0.1626 mg O 162.6 mg 0.1054 mg O 105.4 mg →
Use the data below to detemine the % by mass of Fe to TWO decimal places, if a 0.02 M KMNO4 solution was used for the titration. (MM Fe = 56 g/mol) mass of iron compound (g) 0.691 initial buret reading (mL) 0.77 final buret reading (mL) 16.71
4 You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC H₂O, abated KHP) as the primary standard. KHP (molar mass = 204.22 ganol) has one acidic hydrogen. You prepared solutions of both NaOH and HCI. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 50.75 mL of HCI solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCI solution?
A 100.0 mL water sample was mixed with 25.00 mL of 0.002517 M K₂Cr₂O7 (294.2 g/mol) to oxidize Fe² to Fe³+ The excess K₂Cr₂O7 was back-titrated with 5.30 mL of 0.00949 M Fe²+ on Calculate the concentration of Fe (55.8 g/mol) in the sample in parts per million. *+ Cr₂O7²- + 14H+ 6Fe³+ + 2Cr³+ + 7H₂O ( a. 113 b. 138 C 166 d. 183 e 160 1
1. A 0.5537 g sample containing oxalic acid, H2C2O4 (MM = 90.03 g/mol) required 21.62 mL of 0.09377 M NaOH for titration. Calculate the percent oxalic acid in the sample.Required to answer. Single line text. 2. What mass of solute in milligrams is contained in 26.0 mL of 0.250 M sucrose (MM = 342 g/mol)?Required to answer. Single line text.
Exactly 0.5012g of primary standard KHP (204.22 g/mol) was dissolved in 100.00 ml volumetric flask. A 20.00 ml of that solution was titrated with NaOH which required 8.40 ml to reach phenolphthalein end point. Calculate the molarity of NaoH? 1. 00.2544 M 2. O0.0584 M 3. O0.1023 M 4. 00.1532 M Previoun Next
A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 28.4 mL of HNO3 was required. Given that 0.00966 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction? mol 1 3. 4 C 7 8. +/- х 10 LO
According to the reaction below: if 28.31 mL of KOH with an unknown concentration were titrated using a solution of H2SO4 with a concentration of 0.210 M, and it required 95.41 mL of the H2SO4 solution to react with all of the KOH, what was the initial concentration of the KOH solution in mol/L. H2SO4 +2KOH → 2H2O + K2SO4