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formed in it. It is unsatisfactory in that it does not give full information about the way in which the reaction takes place. For example, it does not suggest that hydrogen is at first formed, and subsequently transformed into water. It is always much more important to remember the steps in a chemical reaction than to remember the equation expressing the complete action; for if these steps in the reaction are understood, the complete equation is easily obtained in the manner just described. ~Salts of nitric acid,--nitrates.~ The salts of nitric acid are called nitrates. Many of these salts will be described in the study of the metals. They are all soluble in water, and when heated to a high temperature undergo decomposition. In a few cases a nitrate on being heated evolves oxygen, forming a nitrite: NaNO_{3} = NaNO_{2} + O. In other cases the decomposition goes further, and the metal is left as oxide: Cu(NO_{3})_{2} = CuO + 2NO_{2} + O. ~Nitrous acid~ (HNO_{2}). It is an easy matter to obtain sodium nitrite (NaNO_{2}), as the reaction given on the previous page indicates. Instead of merely heating the nitrate, it is better to heat it together with a mild reducing agent, such as lead, when the reaction takes place which is expressed by the equation NaNO_{3} + Pb = PbO + NaNO_{2}. When sodium nitrite is treated with an acid, such as sulphuric acid, it is decomposed and nitrous acid is set free: NaNO_{2} + H_{2}SO_{4} = NaHSO_{4} + HNO_{2}. The acid is very unstable, however, and decomposes readily into water and nitrogen trioxide (N_{2}O_{3}): 2HNO_{2} = H_{2}O + N_{2}O_{3}. Dilute solutions of the acid, however, can be obtained. COMPOUNDS OF NITROGEN WITH OXYGEN Nitrogen combines with oxygen to form five different oxides. The formulas and names of these are as follows: N_{2}O nitrous oxide. NO nitric oxide. NO_{2} nitrogen peroxide. N_{2}O_{3} nitrogen trioxide, or nitrous anhydride. N_{2}O_{5} nitrogen pentoxide, or nitric anhydride. These will now be briefly discussed. ~Nitrous oxide~ (_laughing gas_) (N_{2}O). Ammonium nitrate, like all nitrates, undergoes decomposition when heated; and owing to the fact that it contains no metal, but does contain both oxygen and hydrogen, the reaction is a peculiar one. It is represented by the equation NH_{4}NO_{3} = 2H_{2}O + N_{2
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