# A 1.0 sample of an aqueous solution contains0.10 mol of NaCl and 0.10 mol of CaCl2.What is the minimum number of moles ofAgNO3.that must be added to the solution inorder to precipitate all of the Cl ̄ as AgCl(s) ?

Question
Asked May 2, 2019
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A 1.0 sample of an aqueous solution contains
0.10 mol of NaCl and 0.10 mol of CaCl
2.What is the minimum number of moles of
AgNO3.that must be added to the solution in
order to precipitate all of the Cl ̄ as AgCl(s) ?
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Step 1

Given -

Volume of soliution - 1 L

Moles of NaCl in solution = 0.10 mol

Moles of CaCl2 in solution = 0.10 mol

Step 2

Thus, as per the reactions occuring in solution-

Stoichiometrically ,1 mole of NaCl produces 1 mole of Cl‾ ion and 1 mole of CaCl2 produces 2 moles of Cl‾ ions.

Therefore, 0.10 mole of NaCl produces 0.10 mol of Cl‾ ion and 0.10 mol of CaClproduces (2×0.10) moles of Cl‾ ions.

Step 3

When AgNO3 is added to solution containing 0.30 mol of Cl- ions , all these chloride ions react with AgNO3 to form AgCl.

As per balanced equation, 1 mole of Cl- reacts with...

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