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mno 2 + so 2 + h 2 o → mnso 4 (h 2 o) It can also be made by mixing potassium permanganate with sodium hydrogen sulfate and hydrogen peroxide . Manganese sulfate is a by-product of various industrially significant oxidations that use manganese dioxide, including the manufacture of hydroquinone and anisaldehyde .
Ammonium iron(II) sulfate, or Mohr's salt, is the inorganic compound with the formula (NH 4) 2 SO 4 ·Fe(SO 4)·6H 2 O. Containing two different cations , Fe 2+ and NH + 4 , it is classified as a double salt of ferrous sulfate and ammonium sulfate .
In Mn(CH 3) 2 (dmpe) 2, Mn(II) is low spin, which contrasts with the high spin character of its precursor, MnBr 2 (dmpe) 2 (dmpe = (CH 3) 2 PCH 2 CH 2 P(CH 3) 2). [38] Polyalkyl and polyaryl derivatives of manganese often exist in higher oxidation states, reflecting the electron-releasing properties of alkyl and aryl ligands.
The test can distinguish between copper (Cu), iron (Fe), and calcium (Ca), zinc (Zn) or lead (Pb). Sodium carbonate solution is added to the salt of the metal. A blue precipitate indicates Cu 2+ ion. A dirty green precipitate indicates Fe 2+ ion. A yellow-brown precipitate indicates Fe 3+ ion. A white precipitate indicates Ca 2+, Zn 2+, or Pb 2 ...
Manganese(II,III) oxide is the chemical compound with formula Mn 3 O 4. Manganese is present in two oxidation states +2 and +3 and the formula is sometimes written as MnO·Mn 2 O 3. Mn 3 O 4 is found in nature as the mineral hausmannite.
Metallic ions in aqueous solution display many colours: • the red cobalt cation Co 2+ from Co(NO 3) 2 (see § Co) • the orange chromium oxyanion Cr 2 O 2− 7 from K 2 Cr 2 O 7 • the yellow chromium oxyanion CrO 2− 4 from K 2 CrO 4 • the turquoise nickel cation Ni 2+ from NiCl 2
The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.