Question

silver is used to determine the presence of chloride ions in a water sample solution. During a titration procedure 20.2 ml of a 0.10 mol/L Ag+ is used to react with all the chloride ions in the sample. Volume of the water is 10.0mL.

a. write the net-ionic equation for the reaction
b. calculate the mass of Cl in the sample solution
c. calculate the %(m/v) Cl in the sample solution

Answer 1

Ag^+(aq) + Cl^-(aq) ==> AgCl(s)
millimoles = mL x M = 20.2 mL x 0.10 M = 2.02
Therefore, mmoles Cl^- must be 2.02 or 0.00202 moles.
grams Cl^- = mols x molar mass = 0.00202 x 35.456 g/mol = 0.0716 g
% m/v = (g/mL)100 = ?
You should confirm all of the calculations AND look up the atomic mass of Cl. I may not have remembered that correctly.