Top 50 How To Neutralize Ferric Chloride 17120 People Liked This Answer

I’m trying to neutralize Ferric Chloride solution w/Sodium Hydroxide and the chemical manufacturer recommends testing for 7-8 pH. If I buy Pool/Spa pH test strips from a local store, will those work? : chemistry

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• Most searched keywords: Whether you are looking for I’m trying to neutralize Ferric Chloride solution w/Sodium Hydroxide and the chemical manufacturer recommends testing for 7-8 pH. If I buy Pool/Spa pH test strips from a local store, will those work? : chemistry I’m trying to neutralize Ferric Chlore solution w/Sodium Hydroxe and the chemical manufacturer recommends testing for 7-8 pH. Hello! I am using solution to do some PCB etching, and I am trying to figure out how to safely dispose of the chemical after use. They recommend …
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Detoxification Process for a Ferric Chloride Etching Waste | Hazardous Waste and Hazardous Materials

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Ferric Chloride Safety – Beginners Place – Bladesmith’s Forum Board

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• Summary of article content: Articles about Ferric Chloride Safety – Beginners Place – Bladesmith’s Forum Board Just enough to make it slightly alkaline, which is how it neutralizes ferric chlore instantly. By the way, plain tap water also … …
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Neutralizing Ferric Chloride | JerzeeDevil

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how do you all dispose of Ferric Chloride?

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acid base – What is the chemical reaction between Ferric Chloride and Baking Soda – Chemistry Stack Exchange

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Project:Deactivating a ferric chloride solution

Project maintained by Daniel Sikar ~/ dsikaratgmaildotcom.

Deactivating a ferric chloride solution

In practice

Example

A solution that was made with a packet of ferric chloride (FeCl 3 ) crystals weighing 300 grams requires 222 grams of sodium hydroxide (NaOH) to be deactivated.

After deactivation, the neutralised solution will contain iron hydroxide (Fe(OH) 3 ) which is rust and sodium chloride (NaCl) which is common table salt.

Both are innocuous and can be poured down the drain.

Method

Pour the spent ferric chloride solution in a plastic bucket – do not use metal buckets, add about 5 times its volume of water. Dissolve 222 grams of sodium hydroxide in about 3 litres 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 (CuCO 3 ) 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.

In Theory

Ferric chloride reacts with sodium hydroxide turning into ferric hydroxide and sodium chloride.

FeCl 3 + 3 NaOH → Fe(OH) 3 + 3 NaCl

The proportions are:

1 mole of FeCl 3 which is 91,3g reacting with 3 moles of NaOH which is 120g.

The mass of 1 mole is obtained by adding together the atomic masses obtained from the periodic table of elements:

Iron (Fe) has the atomic mass of 55.8 (grams/mole) and Chlorine (Cl) has the atomic mass of 35,5 (grams/mole).

Ferric chloride (FeCl 3 ) 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.

Conversely; Sodium (Na) ~ 23 g/mole, Oxygen (0) ~ 16 g/mole and Hydrogen (H) 1 g/mole totalling 40 grams per mole.

Each mole of FeCl 3 requires 3 moles of NaOH (sodium hydroxide) at 40 grams per mole.

The weight of Na0H required to deactivate the spent FeCl 3 solution is obtained thus:

1.85 * 3 = 5.55 moles of NaOH, at 40 g/mole that will be 5.55 * 40 = 222 grams NaOH.

Detoxification Process for a Ferric Chloride Etching Waste

Abstract

This study deals with the neutralization and detoxification of a spent ferric chloride etching solution from the manufacture of nickel alloy heating elements. In the manufacture of these elements some surface metal is removed by means of a ferric chloride solution that gradually loses its effectiveness due to an excessive build up of nickel and chromium salts. Although the etching waste is not a hazardous waste according to the United States EPA criteria, the state of Missouri includes all etching solutions as hazardous waste. In order to change this spent ferric chloride etching solution from a hazardous waste to an industrial solid waste classification, neutralization tests were performed using three alkaline sources; sodium hydroxide, calcium hydroxide, and sludge from a municipal water treatment plant. Neutralization of the liquid etching waste solution precipitates relatively insoluble metal hydroxide sludges. These sludges were tested according to the EPA Extraction Procedure (EP) toxicity test. Passage of the EP toxicity test allows a waste generator to petition the regulatory agencies for a delisting of the hazardous waste. Results indicate that calcium hydroxide is the most effective and economic means of neutralizing the spent ferric chloride etching solution. A calcium hydroxide addition of the 0.7 kg per liter of waste will neutralize the acidic waste, allow passage of the EP toxicity test for hazardous waste delisting, and produce a solid with a suitable solids content to permit it to be landfilled.

Neutralizing Ferric Chloride

Centaur; you are correct that acids and bases neutralize each other. Actually, they form salts and water. You can tell whether an aqueous solution of a salt will be acidic or basic (alkaline) by looking at what the reactants were.Take ferric chloride. This is a salt formed from ferric oxide and hydrochloric acid (or could be just Fe and HCl). The point is that ferric oxide (rust) is not a very strong base, but hydrochloric acid is a very strong acid; that is to say HCl is nearly completely dissolved into H+ and Cl- ions in water.Thus, ferric chloride is a salt formed from the reaction of a weak base and a strong acid. You would expect this salt to be acidic if dissolved in water, and you would be right. Therefore, you would need a base to neutralize the salt, NOT an acid such as acetic acid (vinegar).Thus, sodium bicarbonate, a weak base (formed from the reaction of sodium hydroxide, a strong base, and carbonic acid, a weak acid), would do the job of neutralizing the ferric chloride.Nathan House; I believe you mispoke yourself when you said ‘ferric acid.’ You meant, I believe, to say an aqueous solution of ferric chloride. Although I must admit it is an acidic solution, and does have ferric ions in it.I would agree emphatically with the suggestion to use a small amount of detergent in with the sodium bicarbonate. This would lower the surface tension of the solution so that it would penetrate the pores of the steel better. Gentle brushing with an old tooth brush wouldn’t hurt either.Hope this helps; I hate to think that I spent all that time in the mid ’60’s in chemistry classes and didn’t learn ANYTHING!Walt

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