Hi!
The first step for this problem is to determine the stoichiometric ratio in which the KIO3 and Na2S2O3 react to form the I2 product:
It turns out that this reaction is a little complicated. Here is a detailed description of the titration reactions. But, in brief:
For every 1 mole of IO3, you get 3 moles of I3
For every 1 mole of I3 you require 2 moles of S2O3
Thus, for every 1 mole of KIO3 that are present you require 6 moles of Na2S2O3
So, lets start by converting 0.1045g of KIO3 to moles:
Next, we multiply this by 6 to determine the required number of moles of Na2S2O3:
Finally, we divide 0.0029 moles of Na2S2O3 by the volume (in Liters) to get the final concentration:
I hope this helps! Please don't forget to rate : )
Titration of the I2 produced from .1045g of primary standard KIO3 required 30.72ml of sodium thiosulfate Calculate t...
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?
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].
In one trial of the standardization of a Na2S2O3 solution, a 10.00 mL volume of 5.00×10-3 M KIO3 is pipetted into a 250 mL Erlenmeyer flask. The solution is titratedto the endpoint with 15.23 mL of the Na2S2O3 solution. What is the molar concentration of this sodium thiosulfate solution?
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 =...
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...
Suppose a student needs to standardize a sodium thiosulfate, Na, S,Og, 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 KIO2 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 concentration of Na,...
Suppose a student needs to standardize a sodium thiosulfate, Na, S,O,, 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 I mL H, SO. The student then titrates the solution with sodium thiosulfate solution in order to determine the exact concentration of...
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?
The concentration of HCl can be determined by titration with a primary standard such as sodium carbonate (Na2CO3). The titration reaction is CO3 2 H H2OCO2 What is the concentration of HCl if 35.5 mL of HCl was needed to to react with 0.201 g of Na2CO3 to reach the end point? concentration:
tion 2 of 2 OAttempt 1 Suppose a student needs to standardize a sodium thiosulfate, Na, S, O,, 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 mlL 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...