# How many ppm of O2 does H2O2 add to water?

• bland
In summary, adding hydrogen peroxide does not add oxygen, oxygen will be produced when the hydrogen peroxide decomposes. To provide 10 ppm in 1 litre of water will require 1000 x 10^-5 = 10^-2 g of oxygen. This will require (10^-2) x 100/47 = 0.02 g of hydrogen peroxide. Using a 6% solution will require 0.02 x 100 / 6 = 0.33g of hydrogen peroxide.
bland
TL;DR Summary
Trying to work out how to raise the oxygen ppm of a litre of water by a measure quantity using hydrogen peroxide.
I'm starting with a litre of distilled water with a dissolved oxygen content of zero ppm, and I wish to raise the ppm of the dissolved O2 to 10ppm or 10mg/L using a 6% solution of H2O2. That is 10 extra molecules of oxygen in a litre!

I've had no luck looking for through web based conversion calculators and other technical papers. So I am reaching out here hoping that someone can explain the correct way to calculate this.

bland said:
That is 10 extra molecules of oxygen in a litre!
No, 10 ppm doesn't mean 10 molecules.

Technically adding hydrogen peroxide you don't add oxygen, oxygen will be produced when the hydrogen peroxide decomposes - which takes time. Kinetics of the process will be a nightmare to describe, as it depends on other dissolved substances catalyzing the reaction.

What you can do is to calculate amount of oxygen that will be produced from the introduced hydrogen peroxide (rather simple stoichiometry), that will help you estimate maximum possible concentration of oxygen after the decomposition (with assumption none of the produced oxygen runs out).

I wanted to work this out just for fun as I am not a real chemist. Molar Mass of hydrogen peroxide is 34, and of oxygen 32. The reaction is 2 H2O2 gives O2. So 68g of hydrogen peroxide give 32g of oxygen, a yield of 32/68 x100=47%.
To provide 10ppm in 1 litre of water will require 1000 x 10^-5 = 10^-2 g of oxygen. This will require (10^-2) x 100/47 = 0.02 g of hydrogen peroxide. Using a 6% solution will require 0.02 x 100 / 6 = 0.33g of hydrogen peroxide.
As this is a very small amount to measure, maybe dilute the hydrogen peroxide a further ten times before measuring the dose.

bland and BillTre
tech99 said:
This will require (10^-2) x 100/47 = 0.02 g of hydrogen peroxide.
OK
tech99 said:
Using a 6% solution will require 0.02 x 100 / 6 = 0.33g of hydrogen peroxide.
Of the hydrogen peroxide solution, to be precise

tech99
tech99 said:
I wanted to work this out just for fun as I am not a real chemist. Molar Mass of hydrogen peroxide is 34, and of oxygen 32. The reaction is 2 H2O2 gives O2. So 68g of hydrogen peroxide give 32g of oxygen, a yield of 32/68 x100=47%.
To provide 10ppm in 1 litre of water will require 1000 x 10^-5 = 10^-2 g of oxygen. This will require (10^-2) x 100/47 = 0.02 g of hydrogen peroxide. Using a 6% solution will require 0.02 x 100 / 6 = 0.33g of hydrogen peroxide.
As this is a very small amount to measure, maybe dilute the hydrogen peroxide a further ten times before measuring the dose.

Okie dokie that is some decent ball park figures to work with, it is indeed a small quantity. thanks.

If your water is open to the atmosphere, then a small amount of air (mostly nitrogen, but about 19% oxygen) will dissolve in the water. To remove it, you will need to boil the water. That also makes it sterile (until the air re-dissolves into the liquid). For fun, buy Clean&Clear or Oxysept used for dis-infecting contact lenses. C&C uses a platinum disc (catalyst) to decompose the H2O2 to water. Oxysept uses catalase, an enzyme, with a pink indicator to decompose the H2O2 to water. You can see the Oxygen bubbling out almost immediately. Process to convert all H2O2 to plain water requires 6 hours. I am a chemist and a contact lens wearer.

Tom.G

## 1. How is ppm of O2 in water affected by the addition of H2O2?

The ppm of O2 in water is directly affected by the addition of H2O2. As H2O2 decomposes, it releases oxygen molecules into the water, increasing the ppm of O2. The amount of O2 added depends on the concentration of H2O2 and the volume of water.

## 2. What is the typical ppm of O2 added to water by H2O2?

The typical ppm of O2 added to water by H2O2 varies depending on the concentration of H2O2 and the volume of water. However, a general estimate is that for every 1% concentration of H2O2, approximately 10 ppm of O2 is added to the water.

## 3. Is the ppm of O2 added by H2O2 permanent or temporary?

The ppm of O2 added by H2O2 is temporary. As H2O2 decomposes, it releases oxygen molecules into the water, increasing the ppm of O2. However, once the H2O2 has completely decomposed, the ppm of O2 will return to its original level.

## 4. Can the ppm of O2 added by H2O2 be measured?

Yes, the ppm of O2 added by H2O2 can be measured using a dissolved oxygen meter. This device measures the amount of oxygen dissolved in water and can provide a reading in ppm.

## 5. Are there any safety concerns when adding H2O2 to water to increase the ppm of O2?

Yes, there are safety concerns when handling H2O2. It is a strong oxidizing agent and can be corrosive to skin and eyes. It is important to follow proper safety precautions when handling and diluting H2O2. Additionally, the increased ppm of O2 in water may also have an impact on aquatic life, so it is important to follow recommended guidelines for H2O2 concentrations in water.

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