Sulfuric acid: Difference between revisions
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'''Sulfuric acid''', also spelled '''sulphuric acid''', is a strong, corrosive acid and reducing agent and is one of the most important chemicals in the chemical industry. Personal protective gear should be worn when using sulfuric acid. | '''Sulfuric acid''', also spelled '''sulphuric acid''', is a strong, corrosive acid and reducing agent and is one of the most important chemicals in the chemical industry. '''Personal protective gear should be worn when using sulfuric acid'''. | ||
== properties and uses of sulfuric acid == | == properties and uses of sulfuric acid == | ||
Sulfuric acid is a strong acid, an oxidizing agent and a dehydrating agent. | Sulfuric acid is a strong acid, an oxidizing agent and a dehydrating agent. It is used to make many soluble phophates for fertilizers, ammonium sulfate and many other chemicals, including drugs. Newly made steel is cleaning with sulfuric acid to remove rust be the steel is coated with a protective layer of zinc, tin or enamel. It is also used in lead sulfate batteries. Many explosives are manufactured using sulfuric acid. | ||
Because it has a high boiling point (330C), it can be used to make other more volatile acids using the appropriate acid salt. Nitric acid can be made by reacting sulfuric acid with [[sodium nitrate]], NaNO<sub>3</sub>. Distilling the resultant nitric acid (BP=86C) drives the reaction towards completion. | |||
: NaNO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → HNO<sub>3</sub> + NaHSO<sub>4</sub> | |||
The explosive nitroglycerin (glyceryl trinitrate), is made by reacting glycerine and nitric acid in the presence of sulfuric acid. '''This reaction is very dangerous, do not attemp.''' | |||
: C<sub>3</sub>H<sub>5</sub>(OH)<sub>3</sub> + 3HNO<sub>3</sub> + (H<sub>2</sub>SO<sub>4</sub> catalyst)→ C<sub>3</sub>H<sub>5</sub>(NO<sub>3</sub>)<sub>3</sub> + 3H<sub>2</sub>O. | |||
Sulfuric acid can be used as a drying agent for gasses that do not react with sulfuric acid by bubbling the gas through sulfuric acid. | |||
== synthesis of sulfuric acid == | == synthesis of sulfuric acid == | ||
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:: 2) 2NOHSO<sub>4</sub> + H<sub>2</sub>O → 2H<sub>2</sub>SO<sub>4</sub> + NO + NO<sub>2</sub> | :: 2) 2NOHSO<sub>4</sub> + H<sub>2</sub>O → 2H<sub>2</sub>SO<sub>4</sub> + NO + NO<sub>2</sub> | ||
== soluble and insoluble sulfate salts == | |||
The soluble salts of sulfate include [[sodium sulfate]] (Na<sub>2</sub>SO<sub>4</sub>)10•H<sub>2</sub>O, [[ammonium sulfate]] (NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub>, [[magnesium sulfate]] (Epsom salt, MgSO<sub>4</sub>•7H<sub>2</sub>O, [[copper sulfate]] ([[blue vitriol]], CuSO<sub>4</sub>•5H<sub>2</sub>O), iron sulfate (FeSO<sub>4</sub>•7H<sub>2</sub>O), zinc sulfate (ZnSO<sub>4</sub>•7H<sub>2</sub>O), potassium aluminum sulfate (alum, KAl(SO<sub>4</sub>)<sub>2</sub>•12H<sub>2</sub>O), ammonium aluminum sulfate (ammonium alum, NH<sub>4</sub>AL(SO<sub>4</sub>)<sub>2</sub>•12H<sub>2</sub>O), and chrome alum (KCr(SO<sub>4</sub>)<sub>2</sub>•12H<sub>2</sub>O). | |||
Barium sulfate is the least soluble sulfate salt and its white precitate is used as a test for sulfate ions. | |||
Revision as of 15:51, 16 January 2008
Sulfuric acid, also spelled sulphuric acid, is a strong, corrosive acid and reducing agent and is one of the most important chemicals in the chemical industry. Personal protective gear should be worn when using sulfuric acid.
properties and uses of sulfuric acid
Sulfuric acid is a strong acid, an oxidizing agent and a dehydrating agent. It is used to make many soluble phophates for fertilizers, ammonium sulfate and many other chemicals, including drugs. Newly made steel is cleaning with sulfuric acid to remove rust be the steel is coated with a protective layer of zinc, tin or enamel. It is also used in lead sulfate batteries. Many explosives are manufactured using sulfuric acid.
Because it has a high boiling point (330C), it can be used to make other more volatile acids using the appropriate acid salt. Nitric acid can be made by reacting sulfuric acid with sodium nitrate, NaNO3. Distilling the resultant nitric acid (BP=86C) drives the reaction towards completion.
- NaNO3 + H2SO4 → HNO3 + NaHSO4
The explosive nitroglycerin (glyceryl trinitrate), is made by reacting glycerine and nitric acid in the presence of sulfuric acid. This reaction is very dangerous, do not attemp.
- C3H5(OH)3 + 3HNO3 + (H2SO4 catalyst)→ C3H5(NO3)3 + 3H2O.
Sulfuric acid can be used as a drying agent for gasses that do not react with sulfuric acid by bubbling the gas through sulfuric acid.
synthesis of sulfuric acid
Sulfuric acid is made be reacting sulfur trioxide with water in an exothermic reaction.
- SO3(g) + H2O(l) → H2SO4(l) + 130 kJ mole-1
In the commercial production of sulfuric acid, the contact process or the lead-chamber process is used. In the contact method, sulfur dioxide is catalytically converted to sulfur trioxide by surface chemistry with fine platinum powder or, more recently, vanadium pentoxide (V2O5). The resulting sulfur trioxide gas is bubbled through sulfuric acid and the addition of water at the correct rate yields 98% acid pulled out.
The lead-chamber process uses sulfur dioxide, oxygen, nitric acid and water vapor are introduced into a lead-lined chamber. White crystals of nitrosulfuric acid (nitronium sulfate), NOHSO4, are formed. The introduction of steam then converts the nitrosulfuric acid to sulfuric acid liberates nitrogen oxides, which can be reused in the first step of the reaction.
- 1) 2SO2 + NO + NO2 + O2 + H2O → 2NOHSO4
- 2) 2NOHSO4 + H2O → 2H2SO4 + NO + NO2
soluble and insoluble sulfate salts
The soluble salts of sulfate include sodium sulfate (Na2SO4)10•H2O, ammonium sulfate (NH4)2SO4, magnesium sulfate (Epsom salt, MgSO4•7H2O, copper sulfate (blue vitriol, CuSO4•5H2O), iron sulfate (FeSO4•7H2O), zinc sulfate (ZnSO4•7H2O), potassium aluminum sulfate (alum, KAl(SO4)2•12H2O), ammonium aluminum sulfate (ammonium alum, NH4AL(SO4)2•12H2O), and chrome alum (KCr(SO4)2•12H2O).
Barium sulfate is the least soluble sulfate salt and its white precitate is used as a test for sulfate ions.