An introduction to the study of inorganic chemistry by unknow

Author:unknow
Language: eng
Format: epub
Tags: Chemistry, Inorganic
Publisher: Columbus, Ohio, Chemical laboratory of the Ohio state university
Published: 1904-03-25T05:00:00+00:00

of that class of substances. It changes blue litmus red, ha^ a sour taste in dilute solutions, and neutralizes bases forming-salts. With potassium hydroxide and sodium hydroxide the reactions are represented by the equations:

HNO3 + KOH = KNO3 + H2O HNO3 + NaOH =: NaNOg + H^O It also acts upon the oxides of most metals, forming a salt and .water as in equations:

PbO + 2 HNO3 = PbCNOg)^ + H^O CuO + 2 HNO3 = Cu(N03)2 + H2O It is one of the strongest acids, by which is meant that it is largely broken up into its ions H and NO3 in solution.

2. Decomposition on Heating. When boiled, or exposed for some time to sunlight, it suffers a partial decomposition according to the equation

2 HNO3 = H2O + 2 NOo + O The substance NOo, called nitrogen peroxide, is a brownish gas which is readily soluble in water and in nitric acid. It therefore dissolves in the undecomposed acid, and imparts a yellowish color to it. Strong nitric acid highly charged with this substance is called fuming nitric acid.

3. Nitric Acid as an Oxidizing Agent. As is shown by its formula, nitric acid contains a large amount of oxygen, and the reaction just mentioned shows that the compound is not a very stable one, easily undergoing decomposition. These properties should make it a good oxidizing agent, and we find that this is the case. Under ordinary circumstances, when acting as an oxidizing agent, it is decomposed according to the equation

2 HNO3 = H^O + 2 NO + 3 O the oxygen being taken up by the substance oxidized, and not set free as is indicated in the equation. Thus if sulphur

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