M2SO43

M2SO43 is not a standard or widely recognized chemical formula in inorganic chemistry. The string could be a typographical error or shorthand for one of several related formulas, such as M2(SO4)3, which would denote a sulfate of a trivalent metal (for example Al2(SO4)3 or Fe2(SO4)3), or MSO4, which would be a sulfate of a divalent metal written without parentheses. It could also intend a hydrated form such as M2(SO4)3·nH2O or MSO4·nH2O. Without clarification, the exact compound cannot be identified with confidence.

If interpreted as M2(SO4)3, this family would comprise sulfates of metals in a +3 oxidation state, with two metal cations balancing three sulfate anions. The sulfate ion (SO4)2− is a tetrahedral anion, and the solid-state structure and hydration state of M2(SO4)3 salts vary with the specific metal. Common examples include aluminum sulfate Al2(SO4)3, iron(III) sulfate Fe2(SO4)3, and chromium(III) sulfate Cr2(SO4)3. Hydrates are common for many sulfates, and aqueous solutions of these salts can be acidic and reactive with water to form hydroxides under certain conditions.

Representative uses and occurrences vary by metal. Aluminum sulfate is widely used in water treatment and paper production as a coagulant. Iron(III) and chromium(III) sulfates have applications in chemistry and materials processing, though some tend to hydrolyze in water and must be handled under appropriate conditions. Sulfates in general are common in minerals; many are soluble to varying extents in water and can form crystalline hydrates.

Synthesis typically involves neutralization or metathesis reactions between sulfuric acid and a metal compound, for example 2 M(OH)3 + 3 H2SO4 → M2(SO4)3 + 6 H2O, with stoichiometry adjusted for the specific metal. Safety and handling depend on the particular metal; some sulfates are relatively benign, while sulfates of toxic metals require care.