Preparation of Acids
- By direct combination of a non metal with hydrogen
e.g. \[{{H}_{2}}+\,C{{l}_{2}}\,\to 2HCl;\,\,{{H}_{2}}+S\to {{H}_{2}}S;\,\,{{H}_{2}}+B{{r}_{2}}\to 2HBr\]
- By reaction between salt and the less concentrated acid
e.g. \[KCl+{{H}_{2}}S{{O}_{4}}\to {{H}_{2}}S{{O}_{4}}+HCl;\,\,NaCl+{{H}_{2}}S{{O}_{4}}\to NaHO{{S}_{4}}+HCl\]
- By action of concentrated nitric acid on non metals.
e.g. \[S+6HN{{O}_{3}}(con)\to {{H}_{2}}S{{O}_{4}}+2{{H}_{2}}O+6N{{O}_{2}}\]
- By dissolving non-metal oxides in water
e.g. \[S{{O}_{3}}+{{H}_{2}}O\to {{H}_{2}}S{{O}_{4}};\,{{N}_{2}}{{O}_{5}}+{{H}_{2}}O\to 2NH{{O}_{3}};\,C{{O}_{2}}+{{H}_{2}}O\to \,{{H}_{2}}C{{O}_{3}}\]
- By action of dilute mineral acids on salts such as chlorides, carbonates sulphates etc.
e.g. \[{{K}_{2}}{{O}_{3}}+{{H}_{2}}S{{O}_{4}}\,(dil)\to {{K}_{2}}S{{O}_{4}}+{{H}_{2}}S{{O}_{4}};\,FeS+{{H}_{2}}S{{O}_{4}}\,(dil)\to FeS{{O}_{4}}+{{H}_{2}}S\]
Properties of Acids
They have sour taste
They turns blue litmus red
III. Dilute mineral acids reacts with metals, above hydrogen in the activity series to liberate hydrogen gas.
\[2Na+2HCl\,(dil)\to 2NaCl+{{H}_{2}}\]
\[Zn+{{H}_{2}}S{{O}_{4}}(dil)\to ZnS{{O}_{4}}+{{H}_{2}}\]
(4) Reaction of Na, K, Ca with acid is explosive.
(5) Hydrogen gas evolved produces "POP"
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