Preparation of Acids, Based and Salts
Category : 10th Class
e.g. \[{{H}_{2}}+\,C{{l}_{2}}\,\to 2HCl;\,\,{{H}_{2}}+S\to {{H}_{2}}S;\,\,{{H}_{2}}+B{{r}_{2}}\to 2HBr\]
e.g. \[KCl+{{H}_{2}}S{{O}_{4}}\to {{H}_{2}}S{{O}_{4}}+HCl;\,\,NaCl+{{H}_{2}}S{{O}_{4}}\to NaHO{{S}_{4}}+HCl\]
e.g. \[S+6HN{{O}_{3}}(con)\to {{H}_{2}}S{{O}_{4}}+2{{H}_{2}}O+6N{{O}_{2}}\]
e.g. \[S{{O}_{3}}+{{H}_{2}}O\to {{H}_{2}}S{{O}_{4}};\,{{N}_{2}}{{O}_{5}}+{{H}_{2}}O\to 2NH{{O}_{3}};\,C{{O}_{2}}+{{H}_{2}}O\to \,{{H}_{2}}C{{O}_{3}}\]
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
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" sound on burning.
But \[Mg\And Mn\] react with very dilute \[HN{{O}_{3}}\] to produce hydrogen gas.
\[Mg+2HN{{O}_{3}}\to Mg{{(N{{O}_{3}})}_{2}}+{{H}_{2}}\,(1%)\]
\[{{K}_{2}}O+2HCl\to 2KCl+{{H}_{2}}O\]
\[MgO+{{H}_{2}}S{{O}_{4}}\to MgS{{O}_{4}}+\,{{H}_{2}}O\]
\[2\,KOH+{{H}_{2}}S{{O}_{4}}\to {{K}_{2}}S{{O}_{4}}+2{{H}_{2}}O\]
\[NaOH+HCl\to MgS{{O}_{4}}+{{H}_{2}}O\]
\[2NaH\,C{{O}_{3}}+{{H}_{2}}S{{O}_{4}}\to N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O+2C{{O}_{2}}\]
\[Zn\,C{{O}_{3}}+2HCl\to ZN\,C{{l}_{2}}+{{H}_{2}}O+C{{O}_{2}}\]
Carbon dioxide gas when passed through line water, turns it to milky due to the formation of calcium carbonate.
\[Ca{{(OH)}_{2}}+C{{O}_{2}}\to CaC{{O}_{3}}+{{H}_{2}}O\]
Acids react with sulphites and hydrogen sulphites to form salt, water and sulphurdioxide
\[{{K}_{2}}S{{O}_{3}}+{{H}_{2}}S{{O}_{4}}\to {{K}_{2}}S{{O}_{4}}+{{H}_{2}}O+S{{O}_{2}}\]
\[NaHS{{O}_{3}}+NaCl\to NaCl+{{H}_{2}}O+S{{O}_{2}}\]
Sulphur dioxide gas also turn lime water milky when passed through it, but is not permanent.
\[MgS+{{H}_{2}}S{{O}_{4}}\to MgS{{O}_{4}}+{{H}_{2}}S\]
\[FeS+2HCl\to FeC{{l}_{2}}+{{H}_{2}}S\]
Hydrogen sulphide gas smells like rotten egg.
Uses of Some Common Acids
Preparation of Bases
\[2Mg+{{O}_{2}}\to 2MgO\]
\[4Na+{{O}_{2}}\to 2N{{a}_{2}}O\]
\[N{{a}_{2}}O+{{H}_{2}}O\to 2NaOH\]
\[MgO+{{H}_{2}}O\to Mg{{(OH)}_{2}}\]
\[2K+2{{H}_{2}}O\to 2KOH+{{H}_{2}}\]
\[Ca+2{{H}_{2}}O\to Ca{{(OH)}_{2}}+{{H}_{2}}\]
\[ZnC{{O}_{3}}\to ZnO+C{{O}_{2}}\]
\[CuC{{O}_{3}}\to CuO+C{{O}_{2}}\]
Sodium and potassium carbonates do not give this reaction
\[2Al(N{{O}_{3}})\to A{{l}_{2}}{{O}_{3}}+6N{{O}_{2}}+3{{O}_{2}}\]
\[CuC{{l}_{2}}+NaOH\to NaCl+Cu{{(OH)}_{2}}\]
\[ZnS{{O}_{4}}+2KOH\to {{K}_{2}}S{{O}_{4}}+Zn{{(OH)}_{2}}\]
\[CuC{{l}_{2}}+NaOH\to NaCl+Cu{{(OH)}_{2}}\]
Properties of Base
III. They react with carbon dioxide in air to form respective carbonate
\[2KOH+C{{O}_{2}}\to {{K}_{2}}C{{O}_{3}}+{{H}_{2}}O\]
\[2NaOH+C{{O}_{2}}\to N{{a}_{2}}C{{O}_{3}}+{{H}_{2}}O\]
The lime water containing \[Ca{{(OH)}_{2}}\], is used for white washing. When left for some time, it reacts with \[C{{O}_{2}}\] in air to form a shiny layer of \[CaC{{O}_{3}}\].
\[NaOH+HN{{O}_{3}}\to NaN{{O}_{3}}+{{H}_{2}}O\]
\[Ca{{(OH)}_{2}}+{{H}_{2}}S{{O}_{4}}\to CaS{{O}_{4}}+2{{H}_{2}}O\]
\[NaOH+N{{H}_{4}}Cl\to NaCl+{{H}_{2}}O+N{{H}_{3}}\]
\[2KOH+{{(N{{H}_{4}})}_{2}}C{{O}_{3}}\to {{K}_{2}}C{{O}_{3}}+2{{H}_{2}}O+N{{H}_{3}}\]
Ammonia has pungent odour. When a glass rod dipped in dilute hydrochloric acid is brought near the mouth of the test tube containing ammonia and white fumes of ammonium chloride is termed.
Hydroxides of zinc, lead and aluminium are amphoteric in nature i.e. they behave both as acids as well as base.
\[Zn{{(OH)}_{2}}+{{H}_{2}}S{{O}_{4}}\to ZnS{{O}_{4}}+2{{H}_{2}}O\]
\[Al{{(OH)}_{3}}+3HN{{O}_{3}}\to Al(N{{O}_{3}})+3{{H}_{2}}O\]
\[Pb{{(OH)}_{2}}+NaOH\to N{{a}_{2}}Pb{{O}_{2}}+2{{H}_{2}}O\]
\[Zn{{(OH)}_{2}}+NaOH\to N{{a}_{2}}Zn{{O}_{2}}+2{{H}_{2}}O\]
Use of Some Common Bases
Preparation of Salts
\[Fe+S\to FeS\] (Iron (ll) Sulphide)
\[Fe+3C{{l}_{2}}\to 2FeC{{l}_{3}}\] (Iron (III) chloride)
\[2Na+C{{l}_{2}}\to 2NaCl\] (sodium chloride)
\[Zn+{{H}_{2}}S{{O}_{4}}\to ZnS{{O}_{4}}+{{H}_{2}}\]
\[Fe+{{H}_{2}}S{{O}_{4}}\to ZnS{{O}_{4}}+{{H}_{2}}\]
\[3Ca+8HN{{O}_{3}}\to 3Cu{{(NaO)}_{2}}+4{{H}_{2}}O+2NO\] (Copper (II) nitrate)
\[N{{a}_{2}}O+2HCl\to 2NaCl+{{H}_{2}}O\]
\[ZnC{{O}_{3}}+2HN{{O}_{3}}\to Zn(N{{O}_{3}})+{{H}_{2}}O+C{{O}_{2}}\]
\[Pb{{(OH)}_{2}}+2HN{{O}_{3}}\to Pb{{(N{{O}_{3}})}_{2}}+2{{H}_{2}}O\]
\[ZnS+2HCl\to ZnC{{l}_{2}}+{{H}_{2}}S\]
\[KHC{{O}_{3}}+HCl\to KCl+{{H}_{2}}O+C{{O}_{2}}\]
\[CaC{{O}_{3}}+{{H}_{2}}S{{O}_{4}}\to CaS{{O}_{4}}+{{H}_{2}}O+C{{O}_{2}}\]
\[CaC{{l}_{2}}+{{K}_{2}}C{{O}_{3}}\to KCl+CaC{{O}_{3}}\]
\[BaS{{O}_{4}}+2NaCl\to BlC{{l}_{2}}+N{{a}_{2}}S{{O}_{4}}\]
Properties of Salts
e.g. Quick lime \[(CaO)\], Concentrated sulphuric acid. Anhydrous calcium chloride etc.
e.g. Sodium Hydroxide \[(NaOH)\], Potassium Hydroxide (KOH), Anhydrous Calcium Chloride.
\[N{{a}_{2}}C{{O}_{3}}.10{{H}_{2}}O\to N{{a}_{2}}C{{O}_{3}}.{{H}_{2}}O+9{{H}_{2}}O\]
Such substances are called efflorescent substances.
e.g.
Common salt turns watery in rainy season. It is because it contains magnesium chloride in traces which is hygroscopic substance.
You need to login to perform this action.
You will be redirected in
3 sec