Project:Deactivating a ferric chloride solution
Project maintained by Daniel Sikar ~/ dsikaratgmaildotcom.
Deactivating a Ferric Chloride solution
A solution that was made with a packet of Ferric Chloride crystals weighing 300 grams requires 222 grams of NaOH to be deactivated.
After deactivating, the neutralised solution will contain Fe(OH)3 (Iron Hydroxide) with is rust and NaCl which is common table salt. Both are innocuous and can be poured down the drain.
Pour in the spent Ferric Chloride solution in a plastic bucket - (do not use metal buckets), add about 5 times its volume with water. Dissolve the 395 grams of Sodium Hydroxide in about 3 liters of water.
In a thin stream, add the Sodium Hydroxide solution to the Ferric Chloride and stir. Once it turns rust coloured it is ready to be discarded.
If not discarded, on standing, the Iron Hydroxide will separate out at the bottom, while at the top, a crust of copper carbonate CuCO3 will form due to the copper from etched circuits.
The iron hydroxide at the bottom is a standard commercial pigment and can be separated off the solution and added to latex paint.
Chemically the reaction is Ferric Chloride reacting to Sodium Hydroxide turning into Ferric Hydroxide and Sodium Chloride.
FeCl3 + 3NaOH -> Fe(OH)3 + 3NaCl
The proportions are:
1 mole of FeCl3 which is 91,3g reacting with 3 moles of Sodium Hydroxide 3NaOH which is 120g.
The mass of 1 mole is obtained by adding together the atomic masses obtained from the periodic table of elements:
Chlorine (Cl) has the atomic mass of 35,5 (grams/mole) and Iron (Fe) has the atomic mass of 55.8 (grams/mole).
Ferric Chloride (FeCl3) will then have the molecular mass of 55.8 * 1 + 35.5 * 3 = 162.3 g/mole.
To find how many moles are contained in 300 grams of Ferric Chloride the calculation is 300/162.3 = 1.85 moles of Ferric Chloride.
These will require 1.85 * 3 = 5.55 moles of NaOH, at 40 g/mole that will be 5.55 * 40 = 222 grams NaOH
contains 1.85 moles. Each mole requires 3 moles of NaOH (Sodium Hydroxide) at 40 grams per mole.