Question

How many milliliters of 0.215 M FeCl3 solution are needed to react completely with 32.7 mL of 0.0509 M AgNO3 solution? The net ionic equation for the reaction is: Ag+(aq) + Cl-(aq) AgCl(s)

mL of FeCl3:

How many grams of AgCl will be formed?

Answer 1

Ans :

The balanced reaction is given as :

FeCl3 + 3AgNO3 = 3AgCl + Fe(NO3)3

Number of moles of AgNO3 = molarity x volume (L)

= 0.0509 x 0.0327

= 0.00166 mol

3 moles of AgNO3 require 1 mol of FeCl3

Number of moles of FeCl3 required = 0.00166 / 3 = 0.00055 mol

0.215 = 0.00055 / V

V = 0.00258 L

= 2.58 mL

So 2.58 millilitres of 0.215 M FeCl3 is needed.

Each mol of AgNO3 forms one mol of AgCl

So number of mol of AgCl formed = 0.00166 mol

Mass of AgCl formed = 0.00166 x 143.3212

= 0.238 grams