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SnO 2 + 2 H 2 SO 4 → Sn(SO 4) 2 + 2 H 2 O. The latter compound can add additional hydrogen sulfate ligands to give hexahydrogensulfatostannic acid. [16] SnO 2 dissolves in strong bases to give "stannates," with the nominal formula Na 2 SnO 3. [11] Dissolving the solidified SnO 2 /NaOH melt in water gives Na 2 [Sn(OH) 6], "preparing salt ...
SnO is amphoteric, dissolving in strong acid to give tin(II) salts and in strong base to give stannites containing Sn(OH) 3 −. [4] It can be dissolved in strong acid solutions to give the ionic complexes Sn(OH 2) 3 2+ and Sn(OH)(OH 2) 2 +, and in less acid solutions to give Sn 3 (OH) 4 2+. [4] Note that anhydrous stannites, e.g. K 2 Sn 2 O 3 ...
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Sodium stannate, formally sodium hexahydroxostannate(IV), is the inorganic compound with the formula Na 2 [Sn(OH) 6].This colourless salt forms upon dissolving metallic tin or tin(IV) oxide in sodium hydroxide and is used as a stabiliser for hydrogen peroxide. [2]
Tin(II) sulfate (Sn S O 4) is a chemical compound. It is a white solid that can absorb enough moisture from the air to become fully dissolved, forming an aqueous solution; this property is known as deliquescence. It can be prepared by a displacement reaction between metallic tin and copper(II) sulfate: [3] Sn (s) + CuSO 4 (aq) → Cu (s) + SnSO ...
Anhydrous SnCl 2 is prepared by the action of dry hydrogen chloride gas on tin metal. The dihydrate is made by a similar reaction, using hydrochloric acid: Sn (s) + 2 HCl (aq) → SnCl 2 (aq) + H 2 (g) The water then carefully evaporated from the acidic solution to produce crystals of SnCl 2 ·2H 2 O.
This is illustrated in the image here, where the balanced equation is: CH 4 + 2 O 2 → CO 2 + 2 H 2 O. Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. This particular chemical equation is an example of complete combustion. Stoichiometry measures these ...
In chemistry, the term stannate or tinnate refers to compounds of tin (Sn). Stannic acid (Sn(OH) 4 ), the formal precursor to stannates, does not exist and is actually a hydrate of SnO 2 . [ 1 ] The term is also used in naming conventions as a suffix; for example the hexachlorostannate ion is SnCl 2−