Asked by vicky
25ml of 0.01M KIO3 solution were put to react with an excess of KI. 32.04ml of the sodium thiosulfate solution were needed to titrate the triiodide ions that were present .
What is the molar concentration of thiosulfate in the solution?
What is the molar concentration of thiosulfate in the solution?
Answers
Answered by
DrBob222
I have not used the triiodide ion (I3^-) below but you may convert to that if you wish.
KIO3 + 5KI + 3H2SO4 ==> 3H2O + I2 + 3K2SO4
2S2O3^2- + I2 ==> S4O6^2 + 2I^-
mols KIO3 = M x L = ?
mols I2 produced = 3 x that = ?
mols S2O3^2- needed = 2 x mols I2 = ?
Then M S2O3^2- = mols S2O3^2-/L S2O3^2- = ?
KIO3 + 5KI + 3H2SO4 ==> 3H2O + I2 + 3K2SO4
2S2O3^2- + I2 ==> S4O6^2 + 2I^-
mols KIO3 = M x L = ?
mols I2 produced = 3 x that = ?
mols S2O3^2- needed = 2 x mols I2 = ?
Then M S2O3^2- = mols S2O3^2-/L S2O3^2- = ?
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