Suppose a 2.95 g of potassium iodide is dissolved in 350. ml of a 62.0 m m aqueous solution of silver nitrate. calculate the final molarity of iodide anion in the solution. you can assume the volume of the solution doesn't change when the potassium iodide is dissolved in it. be sure your answer has the correct number of significant digits

Answer : The final molarity of iodide anion in the solution is 0.0508 M.

Explanation :

First we have to calculate the moles of and .

Molar mass of KI = 166 g/mole

and,

Now we have to calculate the limiting and excess reagent.

The given chemical reaction is:

From the balanced reaction we conclude that

As, 1 mole of KI react with 1 mole of

So, 0.0178 mole of KI react with 0.0178 mole of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and KI is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of

From the reaction, we conclude that

As, 1 mole of react to give 1 mole of

So, 0.0178 moles of react to give 0.0178 moles of

Thus,

Moles of AgI = Moles of anion = Moles of cation = 0.0178 moles

Now we have to calculate the molarity of iodide anion in the solution.

Therefore, the final molarity of iodide anion in the solution is 0.0508 M.

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