A solution of sodium thiosulfate, Na2S2O3, is 0.7707 M. 7.42 mL of this solution reacts with...
A solution of sodium thiosulfate, Na2S2O3, is 0.7707 M. 7.42 mL of this solution reacts with 24.81 mL of I2 solution. What is the molarity of the I2 solution?
2(Na2S2O3) + I2↔Na2S4O6 + 2(NaI)
20.28 mL of the I2 solution from above is required to titrate a sample containing As2O3. Calculate the mass of As2O3 (197.8 g/mol) in the sample.
As2O3 + 5(H2O) + 2I2 → 2(H3AsO4) + 4HI
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A solution of sodium thiosulfate,
Na2S2O3, is 0.7707 M. 7.42 mL of
this solution reacts with...
balance: KIO3(aq) + KI(aq) + H2SO4(aq) -----> I2(aq) + K2SO4(aq) I2(aq) + Na2S2O3(aq) ------> NaI(aq) + Na2S4O6(aq) &nb
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?
If you have 275 mg of sodium thiosulfate in 20 mL of water, and 14.8 mL...
If you have 275 mg of sodium thiosulfate in 20 mL of water, and 14.8 mL of this solution was required to titrate 104 mg of iodine in 20 mL of solution, what is the amount in mg of Na2S2O3 that is required to completely reduce the 104 mg of I2?
A chemist must prepare 700.mL of 2.00M aqueous sodium thiosulfate Na2S2O3 working solution. He'll do this...
A chemist must prepare 700.mL of 2.00M aqueous sodium thiosulfate Na2S2O3 working solution. He'll do this by pouring out some 3.15mol/L aqueous sodium thiosulfate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the sodium thiosulfate stock solution that the chemist should pour out. Round your answer to 3 significant digits.
What is the mass of sodium thiosulfate (Na2S2O3) needed to add to a solution in order...
What is the mass of sodium thiosulfate (Na2S2O3) needed to add to a solution in order to successfully dissolve 40 mg of silver iodide in 200.0 mL of water
Suppose you need to standardize a sodium thiosulfate solution for a titration experiment. To do so,...
Suppose you need to standardize a sodium thiosulfate solution for a titration experiment. To do so, you will react it with a solution of iodine. You add a 1.00 mL aliquot of 0.0200 M KIO3 solution to a flask, followed by 3 mL of distilled water, 0.2 g of solid KI, and 1 mL H2SO4. You then titrate the solution with sodium thiosulfate solution in order to determine the exact concentration of Na2S2O3. The end point of the titration is...
A 10.00 ml sample of .0.0100 M KIO3 was titrated against a solution of sodium thiosulfate...
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].
Iodine, I2I2, reacts with aqueous thiosulfate ion in neutral solution according to the balanced equation I2(aq)+2S2O2−3(aq)→S4O2−6(aq)+2I−(aq)I2(aq)+2S2O32−(aq)→S4O62−(aq)+2I−(aq)....
Iodine, I2I2, reacts with aqueous thiosulfate ion in neutral solution according to the balanced equation I2(aq)+2S2O2−3(aq)→S4O2−6(aq)+2I−(aq)I2(aq)+2S2O32−(aq)→S4O62−(aq)+2I−(aq). How many grams of I2 are present in a solution if 33.65 mL of 0.135 M Na2S2O3 solution is needed to titrate the I2 solution?
I am doing a titration lab using sodium thiosulfate pentahydrate to determine an amount if iodine....
I am doing a titration lab using sodium thiosulfate pentahydrate to determine an amount if iodine. I'm having issues setting up the balanced equation to determine the mole ratio of iodine to thiosulfate. I used an approximate .080M solution of Sodium Thiosulfate and then titrated into a flask containing 25mL of KIO3, 20mL H2SO4 and 2g KI. Final mL of Sodium Thiosulfate used to complete titration was 37.36mL of Na2S2O3 5H20. I then did the same process for a 25mL...
Government and industry analysts routinely measure the quantity of ascorbic acid (vitamin C, C6H8O6) in commercial...
Government and industry analysts routinely measure the quantity of ascorbic acid (vitamin C, C6H8O6) in commercial products such as fruit juices and vitamin tablets. The ascorbic acid reacts with excess iodine, and the amount of I2 remaining is determined with sodium thiosulfate (Na2S2O3). It is suspected by the Montreal Fraud Division that a prominent natural foods importer is defrauding his customers by claiming that his vitamin C tablets contain 45% of the active ingredient ascorbic acid. In one analysis, a...
Sodium carbonate (MM=105.988 g/mol) is a primary standard base that reacts with hydrochloric acid as follows:
Sodium carbonate (MM=105.988 g/mol) is a primary standard base that reacts with hydrochloric acid as follows: Na2CO3 + 2HCI → 2NaCl + H2O + CO2(g) If 39.09 mL of an HCl solution were required to titrate a solution containing 287.5 mg of primary standard Na2CO3, calculate the molarity of the HCl solution.
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