KIO3 + 6 Na2S2O3 + 6 H+ => KI + 3 Na2S4O6 + 6 Na+ + 3 H2O
Moles of KIO3 = volume x concentration of KIO3
= 10.00/1000 x 5.00 x 10-3 = 5.00 x 10-5 M
Moles of Na2S2O3 = 6 x moles of KIO3
= 6 x 5.00 x 10-5 = 3.00 x 10-4 mol
Concentration of Na2S2O3 = moles/volume in L of Na2S2O3
= 3.00 x 10-4/0.01523
= 0.0197 M = 1.97 x 10-2 M
Standardization of Sodium Thiosulfate Titrant Weight of KIO3 = 1.5062 g; Concentration of KIO3 (M) = 0.0141 M T1: Initial = 0.70 mL; Final = 29.60 mL; Volume of Titrant = 28.90 mL T2: Initial = 2.10 mL; Final = 30.70 mL; Vol. of Titrant = 28.60 mL T3: Initial = 2.20 mL; Final = 30.20 mL; Vol. of Titrant = 28.00 mL Vitaminc C Analysis Trial 1: Initial = 1.60 mL; Final = 15.70 mL; Vol. of Titrant =...
doing experiment about standardization of 0.0025M
sodium thiosulphate solution,
can someone tell me how this formula (calculating exact conc of
Na2S2o3) (at the bottom) comes ?
Data: (10 marks) Part 1: Standardization of 0.0025M sodium thiosulphate solution No. of drops of 0.0025 M sodium thiosulphate solution Solution Trial 1 Trial 2 Trial 3 Average 1 mL of potassium iodate solution + 0.2 mL 3 M HCI + 1 mL D.I. water + 3 drops of starch 2) 22 121.67 N...
A 10.00 ml sample of .0.0100 M KIO3 was titrated against a solution of sodium thiosulfate to standardize it. The initial buret volume reading was 0.07 ml. The final buret reading was 6.54 ml. Calculate the [Na2S2O3].
Suppose you analyze a 34.7 g sample of bleach and determine that there are 2.03 g of sodium hypochlorite present What is the percent of sodium hypochlorite in the bleach sample? Suppose in an experiment to determine the amount of sodium hypochlorite in bleach, 0.0000157 mol KIO, were titrated with an unknown solution of Na2S2O3 and the endpoint was reached after 14.63 mL What is the concentration of the Na2S2O3 solution, in M? Suppose, in an experiment to determine the...
DATA SHEET Overall Stoichiometric Equations 1. Results and Observations 2. Unknown No.:l Concentration of standard Na2S&O3 solution, M 0.020(0 Trial 3 Trial 2 Trial 1 13.22 33.97 o.0.20 1311 Initial burette reading, mL 13.09 Final burette reading, mL (0.21 Volume of NAS2O3 used, mL Amount of NA2S2O3 used, mol Amount of Cu2 in unknown sample, mol L0.00 10. 00 10.00 Volume of original Cu solution used, mL in original solution, M Concentration of Cu Average Concentration of Cu2, M Procedure...
please type answer or fill in the blanks PLEASE
UU ANITOUESTIONS EXPERIMENT 10 PRE-LABORATORY STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If...
balance: KIO3(aq) + KI(aq) + H2SO4(aq) -----> I2(aq) + K2SO4(aq) I2(aq) + Na2S2O3(aq) ------> NaI(aq) + Na2S4O6(aq) Assume that 1.1 mL of the above potassium iodate solution is measured and that 2.20 mL of the unstandardized sodium thiosulfate is required to reach the endpoint. What is the molarity (M), now standardized, sodium thiosulfate?
QUESTIONS 1. Determine the concentration of the HCL solution from the data for the standardization of the HCL with the Na2CO3 2. using your data, calculate the moles and mass of acetylsalicylic acid in each tablet (molar mass=180.16g/mol) 3. Using your data, calculate the % by mass of aspirin in the tablet DATA: 1. Make two solutions; Add 1 tablet of aspirin to an erlenmeyer flask 2. using a 50mL pipette, add 50.0mL of NaOH to the tablets in the...
Suppose a student needs to standardize a sodium thiosulfate, Na, S, O3, solution for a titration experiment. To do so, he or she will react it with a solution of iodine. The student adds a 1.00 mL aliquot of 0.0200 M KIO, solution to a flask, followed by 3 mL of distilled water, 0.2 g of solid KI, and 1 mL H, SO . The student then titrates the solution with sodium thiosulfate solution in order to determine the exact...
(a) Potassium iodate solution was prepared by dissolving 1.022 g of KIO3 (FM 214.00) in a 500 mL volumetric flask. Then 50.00 mL of the solution was pipetted into a flask and treated with excess KI (2 g) and acid (10 mL of 0.5 M H2SO4). How many millimoles of I3− are created by the reaction? (b) The triiodide from part (a) reacted with 37.54 mL of Na2S2O3 solution. What is the concentration of the Na2S2O3 solution? (c) A 1.223...