The amount of i−3(aq) in a solution can be determined by titration with a solution containing a known concentration of s2o2−3(aq) (thiosulfate ion). the determination is based on the net ionic equation 2s2o2−3(aq)+i3(aq)⟶s4o2−6(aq)+3i−(a q) given that it requires 29.6 ml of 0.260 m na2s2o3(aq) to titrate a 30.0 ml sample of i−3(aq), calculate the molarity of i−3(aq) in the solution.

Answer : The molarity of in the solution is, 0.128 M

Explanation :

The given balanced chemical reaction is,

First we have to calculate the moles of .

Conversion used : (1 L = 1000 ml)

Now we have to calculate the moles of .

From the balanced chemical reaction, we conclude that

As, 2 moles of react with 1 mole of

So, 0.007696 moles of react with mole of

The moles of = 0.003848 mole

Now we have to calculate the molarity of .

Now put all the given values in this formula, we get:

Therefore, the molarity of in the solution is, 0.128 M

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