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Magnesium has many different purposes and consequently may end up in water in many different ways. Chemical industries add magnesium to plastics and other materials as a fire protection measure or as a filler. It also ends up in the environment from fertilizer application and from cattle feed. Magnesium sulphate is applied in beer breweries, and magnesium hydroxide is applied as a flocculant in wastewater treatment plants.
Magnesium is also a mild laxative. Magnesium alloys are applied in car and plane bodies. During World War II magnesium was applied in fire bombs, to cause major fires in cities. The development of these bombs introduced a method to extract magnesium from seawater. Magnesium is a dietary mineral for any organism but insects. It is a central atom of the chlorophyll molecule, and is therefore a requirement for plant photosynthesis.
Magnesium cannot only be found in seawater, but also in rivers and rain water, causing it to naturally spread throughout the environment. Three magnesium isotopes occur naturally, which are all stable and consequently not radioactive. There are also eight instable isotopes. Guidelines for magnesium content in drinking water are unlikely, because negative human and animal health effects are not expected.
Environmental problems indirectly caused by magnesium in water are caused by applying softeners. As was described earlier, hardness is partially caused by magnesium.
Calcium and magnesium ions particularly calcium negatively influence cleansing power of detergents, because these form nearly insoluble salts with soap.
This used to be phosphates, but it was discovered that these where hardly biodegradable, and caused eutrophication. These substances do not cause eutrophication and are not toxic. Nitriloacetic acid NTA may be mutagenic, and is difficult to remove during water purification. Zeolite A increases the amount of sludge.
Additionally, other complexing agents such as ethylenediaminetetraacetic acid EDTA have the audacity to remove metals from compounds that are otherwise difficult to decompose. As the hydrogen gas bubbles out of the water it mixes with atmospheric oxygen. The intense heat ignites the hydrogen-oxygen mixture and the mixture continues to burn possibly explosively depending upon the quantities involved as long as hydrogen continues to be generated.
To my knowledge, neither of these metals "burn" underwater. The word burn generally suggests that something reacts with oxygen. As others have stated above, these very active metals will react with water by displacing hydrogen as H 2. The hydrogen definitely will react with oxygen assuming that enough heat is evolved to start the reaction very likely for sodium, less so for magnesium.
Sign up to join this community. The best answers are voted up and rise to the top. Stack Overflow for Teams — Collaborate and share knowledge with a private group. Create a free Team What is Teams? Learn more. How can metals like magnesium and sodium burn underwater?
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