# chemistry

posted by .

in an experiment 5.00ml of 0.1440 mol L^1- aqueos KIO3 was reacted with an excess of aqueous iodide and the molecular iodine I2, Formed was titrated against 0.1000mol L^1- aqueous S2O3^2- the equation for the titration reaction is:

I2(aq)+ 2 S2O3^2-(aq)---->S4O6^2-(aq)+ 2I^-1(aq)

determine the molar ratio of iodine molecules by dividing each mole quantity by the lowest mole quantity. express this as a ratio of integers

IO3- : I2

using this ratio balance the equation please

__IO3^-(aq) + ____ I^-(aq)+____H^+(aq)------>_____ I2(aq)+_____H2O(l)

• chemistry -

I would do it this way.
moles KIO3 = M x L = 0.144 x 0.005 = 0.00072 moles KIO3.
moles S2O3^2- = M x L = 0.1000 x 0.043 = 0.0043 moles S2O3^2-. Convert that to moles I2.
moles I2 = 0.0043 moles S2O3^2- x (1 mole I2/2 moles S2O3^-) = 0.0043 x (1/2) - 0.00215 moles.
So the ratio IO3^- to I2 = 0.00072:0.00215.
To find the ratio in small whole numbers, the easy way to do it is to divide the smaller number by itself, then divide the other number by the same value.
IO3 = 0.00072/0.00072 = 1.000
I2 = 0.00215/0.00072 = 2.986 which rounds in whole numbers to 3.000. (The difference is in your titration. That may have been slightly different than exactly 43.0 mL).
Knowing 1 IO3 = 3 I2, put 1 for the coefficient for IO3, place 3 for I2, then balance the remainder of the equation by inspection. You should get
IO3^- + 5I^- + 6H^+ ==> 3I2 + 3H2O

## Similar Questions

1. ### Chemistry

Hi, I'm really having trouble this this chemistry problem. I have the answers; however I don't have extensive knowledge about titrations and I'm struggling with working it out. If anyone could suggest how to work this out (or even …
2. ### Chemistry

According to the following reaction, how many moles of hydrogen iodide will be formed upon the complete reaction of 30.0 grams of hydrogen gas with excess iodine?
3. ### chemistry

Am doing a lab report on the determination of the product of a redox reaction: the reaction of bromate and hydroxylammonium ions. here is the lab Experiment: In this experiment you will determine the equation of a redox reaction by …
4. ### Chemistry

A 2.50 gram sample of bronze was dissolved in sulfuric acid. The copper in the sample reacted with sulfuric acid to form copper sulfate. Cu (s) +2 H2SO4 (aq) -> CuSO4 (aq) +2 H2O (l) The copper sulfate formed in this reaction was …
5. ### chemistry

If 380. mL of 0.4294 M aqueous CaBr2 and 250. mL of 0.5880 M aqueous SO42- are reacted stoichiometrically according to the equation, how many mol of CaBr2 remained?
6. ### Chemistry

For idometric titration of copper, why is HCl added to KIO3 and then titrated immediatedly?
7. ### chemistry

in an experiment 5.00ml of 0.1440 mol L^1- aqueos KIO3 was reacted with an excess of aqueous iodide and the molecular iodine I2, Formed was titrated against 0.1000mol L^1- aqueous S2O3^2- the equation for the titration reaction is: …
8. ### chemistry

in an experiment 5.00ml of 0.1440 mol L^1- aqueos KIO3 was reacted with an excess of aqueous iodide and the molecular iodine I2, Formed was titrated against 0.1000mol L^1- aqueous S2O3^2- the equation for the titration reaction is: …
9. ### Chemistry 101

Write the molecular, total ionic, and net ionic, for the reaction. 1). Aqueous sodium carbonate is reacted with aqueous nickle (11) chloride. 2). Aqueous potassium hydroxide is mixed with aqueous hydrochloric acid.
10. ### Chemistry

Aqueous sulfurous acid H2SO3 and aqueous sodium chloride are formed by the reaction of aqueous sodium sulfite Na2SO3 and aqueous hydrochloric acid HCl . Write a balanced chemical equation for this reaction.

More Similar Questions