Question

a 1.0 l sample of an aqueous solution contains 0.10 mol of nacl and 0.10 mol of cacl2. 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) ? (assume that agcl is insoluble.) responses 0.10 mol 0.10 mol 0.20 mol 0.20 mol 0.30 mol 0.30 mol 0.40 mol 0.40 mol 0.60 mol

Answer 1

The minimum number of moles of AgNO3 that must be added to precipitate all of the Cl- ions is 0.20 mol.

Step-by-step explanation:

To precipitate all of the Cl- ions as AgCl(s), we need to determine the limiting reactant between NaCl and CaCl2. The number of moles of Cl- ions in 0.10 mol of NaCl is 0.10 mol, while the number of moles of Cl- ions in 0.10 mol of CaCl2 is 0.20 mol (since CaCl2 has two Cl- ions per formula unit). Therefore, the minimum number of moles of AgNO3 that must be added to the solution to precipitate all of the Cl- ions as AgCl(s) is 0.20 mol.