Hydrogen peroxide (H2O2) is a highly reactive compound that readily decomposes, especially at high concentrations. Achieving 100% pure and concentrated hydrogen peroxide is extremely challenging due to its unstable nature. However, there have been reports of achieving relatively high concentrations of hydrogen peroxide under specific conditions.
Historically, a chemist named Richard Wolffenstein claimed to have prepared 100% pure hydrogen peroxide in the early 20th century. However, his claims were later debunked, and it was discovered that the hydrogen peroxide he produced was not actually pure.
Today, commercially available hydrogen peroxide solutions typically range from 3% to 35% concentrations, with the most common concentrations being 3% (household hydrogen peroxide) and 30% (industrial-grade hydrogen peroxide).
To obtain higher concentrations of hydrogen peroxide, various stabilizers are added to prevent its decomposition. Stabilizers such as stabilizing agents, stabilizing salts, or reaction inhibitors are commonly used to extend the shelf life and prevent the spontaneous decomposition of hydrogen peroxide.
Attempting to prepare or handle highly concentrated hydrogen peroxide (above 70-90%) can be extremely dangerous due to its explosive nature and the risk of unintended decomposition. Specialized equipment and expertise are required to handle and store high-concentration hydrogen peroxide safely.
In summary, while achieving 100% pure and concentrated hydrogen peroxide is exceptionally difficult due to its inherent instability, commercially available solutions provide concentrations up to 35%. Handling highly concentrated hydrogen peroxide is hazardous and requires specialized knowledge and precautions.