What are the sulfite and bisulfite ions, and what are they used for?
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Sulfites (also sulphite) are compounds that contain the sulfite ion (SO3)2−. They are often used as preservatives in wines (to prevent spoilage and oxidation), dried fruits, and dried potato products.\n\nThe bisulfite ion is the HSO3− ion. It is the conjugate base of sulfurous acid, H2SO3. Salts containing the HSO3− ion are bisulfite [salt]s It is a weakly acidic substance which has a pKa of 6.97. It can be found in acid compounds used in high school science experiments and not much use anywhere else
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Methylamine (CH3NH2) and methylammonium chloride (CH3NH3Cl) would be a good buffer in both are in solution together in appreciable concentrations.\n\nNitrates, chlorides, and sulfates (either as acids or salts) will not act as buffers as those anions have no tendency to act as bases (they are the anions from strong acids, which are "strong" because they dissociate completely in solution).  The same with alkali metal hydroxides, which are strong bases.
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There really is not a set formula, as the -ite anions don't have a set formula themselves (PO3 2- for phosphite, NO2- for nitrite, SO3 2- for sulfite, Cl02- for chlorite, etc.)
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8. SO3 + H2O --> H2SO4 (sulphuric acid)\n9. Nitric acid - reducing agent\n    Sulphuric acid - concentrated H2SO4 can be used a drying agent, catalyst (in esterification); otherwise, in manufacturing of fertilizers, detergents, and as a battery acid in cars\n    Phosphoric acid - no idea...\n    Carbonic acid - in making carbonated drinks\n\nHope this helps :)
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Do not capitalize the spelled-out names of chemical elements and compounds. When using symbols, use capital letters but no periods.\n\ncadmium Cd\niron         Fe\nsulfuric acid H2 SO4
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lead (IV) sulfate\nLead is a transition metal with an oxidation state of +4 in this molecule\nSulfate is a polyatomic ion made up of one sulfur atom and four oxygen atoms with a charge of -2\nIn order to have a neutral molecule there has to be one lead atom and two sulfate ions giving the following composition:\n1 Pb (lead)\n2 S (sulfur)\n8 O (oxygen)
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In PbSO4 the Pb is +2 and the SO4 group is -2. \nThe O in SO4 is -2 so the sulphur must be +6 (the four oxygens add up to -8 and for the SO4 group to be -2 the sulphur must be +6)\nThe formula for CaOCl2  IS  correct. The Ca is +2 and the OCl2 group -2 as O is usually -2 it would suggest that each chlorine is 0. This anomaly is because the OCl2 is known as a disproportionate ion (having too much chlorine).\nIn (NH4)2SO4  each NH4 group is +1 and the SO4 is -2.\nSo as each H = +1  the N is -3. The SO4 has the same oxidation numbers as in PbSO4 above.\nIn working out oxidation numbers we assume that certain elements have fixed numbers O is -2,  Cl is -1,  H is +1  and alkali metals like sodium and potassium are +1. The complete compound must add up to zero.
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There are a lot of sites that have info.  Search for "formula writing polyatomic ions".\nIf you have a list of polyatomic ions like "SO4", "SO3", "PO4", etc. you will see that they have specific charges associated with them.  SO4 and SO3 both have a negative 2 charge.  Hydrogen has a +1 charge.  A compound must be neutral so you need 2 H to pair with one SO4.  +2-2=0.\nPO4 has a negative 3 charge, so you'd need 3 H+ to offset the 3 negatives.  H3PO4.\n\nAs far as naming them, search for "naming chemical compounds"  The examples you are asking about are actually acids, so you might need to look up "naming acids".
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Nickel (II) oxide, sulphur dichloride, and chlorine\n\n2NiCl2 + S02 ---> SCl2 + 2NiO + Cl2
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It is used to - \nsupply zinc in animal feeds, fertilizers, and agricultural sprays. \n\nZnSO4·7H2O is used in making lithopone, \nin coagulation baths for rayon, \nin electrolytes for zinc plating, \nas a mordant in dyeing, \nas a preservative for skins and leather \nand in medicine as an astringent and emetic.\n\nZinc sulphate can be used in the eye as an astringent to relieve over production of tears. \n\nThey can be particularly useful in those suffering from eye infections, in which watery eyes can be a problem.
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H2SO4 + 2NaOH ----> 2H2O + Na2SO4\n\nYOU MUST SEPARATE AND CANCEL THE COMMON IONS (AQUEOUS ONES)
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Barium Sulfate — BaSO4. It is extremely insoluble in water and will form a white precipate.
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try this site.  if you ever need to look up other chemicals, etc. search for msds b/c that is where all the info on storage, etc will be.\n\nhttp://www.chem.tamu.edu/class/majors/msdsfiles/msdsleadsulfate.htm
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NA2SO4,KOH,AGCL,CA(NO3)2 ARE SOLUBLE.AND HG2BR2 AND CDS IS INSOLUBLE.
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Hydrogen\n\nSODIUM BISULFATE\n\nSynonyms: Sodium hydrogen sulfate; sodium acid sulfate; sulfuric acid, monosodium salt, monohydrate \nCAS No.: 7681-38-1 (Anhydrous) \nMolecular Weight: 138.08 \nChemical Formula: NaHSO4 . H2O \nProduct Codes: \nJ.T. Baker: 3534 \nMallinckrodt: 7432
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sulphuric acid ------- king of acids\npreparation ---------- contact process\nfor making it dilute we must put acid to water and not water to acid as it may explode \nit is used as a dehydrating agent
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1) COPPER CARBONATE + SULPHURIC ACID  GIVES COPPER SULPHATE +WATER + CARBONDIOXIDE \n2) COPPER + SULPHURIC ACID GIVES COPPER SULPHATE