Nitric acid and hydrochloric acid

Methods for preparation of Nitric acid and hydrochloric acid ,its properties and uses .

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2. NITRIC ACID AND
HYDROCHLORIC ACID
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3. NITRIC ACID
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4. INTRODUCTION
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Nitric acid is a colorless liquid that is used in the manufacture of inorganic and organic nitrates
and nitro compounds for fertilizers, dye intermediates, explosives, and many different organic
chemicals.
It is a strong oxidizing agent and can oxidize metals and nonmetals easily.
It is a strong, monoprotic acid and is almost completely ionized in aqueous solution. Nitric acid
is a resonance-stabilized acid allowing it to share its electrons among its own bonds.
Structure:

5. PROPERTIES
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Molar mass: 63g/mol
Color: Pure nitric acid is a colorless liquid but commercial nitric acid may be yellowish brown
due to presence of dissolved nitrogen dioxide.
Odour: Nitric acid is a fuming & hygroscopic liquid.
Acidity: Nitric acid is a strong acid and dissociates very highly and is very corrosive. Ka value
is 28.
Taste: It is sour in taste due to acidic in nature.
Density:1.513gcm
-3
at 20
°
C.

6. TYPES OF NITRIC ACID
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Strong nitric acid:
Density; 1.4; Percentage Concentration; 65% HNO
3.
Fuming nitric acid:
A red liquid made by passing NO
2 gas through concentrated HNO
3.
Concentrated nitric acid:
Density 1.5; Percentage Concentration; 98% HNO
3.

7. PREPARATION METHODS
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CHILE SALTPETRE METHOD BY NANO3
BRIKLAND EYDE’S METHOD BY USING AIR
OSTWALD’S METHOD BY USING AMMONIA

8. OSTWALD’S METHOD
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Three steps method:
Oxidation of ammonia NH
3
Oxidation of nitric oxide
Absorption of NO
2

NH3 is oxidized into NO by air at 800 C in presence of Pt (Platinum) catalyst with 10% Rh
content.

9. RAW MATERIALS
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Ammonia
Water
Air
Catalyst (platinum-rhodium gas)

10. FIRST STEP
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Primary oxidation (formation of nitric acid):
Oxidation of nitric acid is carried out in catalyst chamber in which one part of ammonia
and eight parts of oxygen by volume are introduced. The temperature of chamber is
about 600°C. This chamber contains a platinum gauze which serves as a catalyst.
Chemistry of primary oxidation:
Oxidation of ammonia is reversible and exothermic process. Therefore according to Le-
Chatelier’s principle, decrease in temperature favors the reaction in forward direction. In
primary oxidation, 95% of ammonia is converted to nitric oxide(NO).
4NH
3 + 5O
2 4NO + 6H
2O

11. SECOND STEP
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Secondary oxidation (formation of nitrogen dioxide):
Nitric oxide gas obtained by the oxidation of ammonia, is very hot. In order to reduce its
temperature, it is passed through aat exchanger where the temperature of nitric oxide is reduce
to 150°C. Nitric oxide after the cooling, is transferred to another oxidizing tower where at about
50°C, it is oxidizing to NO
2
2NO + O
2 2NO
2

12. FINAL STEP
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Absorption of NO
2
( formation of HNO
3):
Nitrogen dioxide from secondary oxidation chamber is introduced into special absorption tower.
NO
2 gas passed through the tower and water is showered over it. By the absorption, nitric acid is
obtained.
3NO
2 + H
2O 2HNO
3 + NO
Nitric acid obtained is very dilute. It is recycled in absorption tower so that more and more NO
2
get
absorbed. HNO
3 after recycle becomes about 68% concentrated.
In order to increase the concentration of HNO
3, vapors of HNO
3 are passed over concentrated
H
2SO
4. Being a dehydrating agent, H
2SO
4 absorbs water from the HNO
3 and concentrated
HNO
3 is obtained.

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14. FLOW SHEET
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BIRKLAND EYDE PROCESS
In this process the nitrogen and oxygen of the air combine to give
nitric oxide in an electric arc at temperature 3000
At 600 0C NO combine with O2 to give NO2
Nitrogen dioxide is absorbed in water to give dilute nitric acid
along with nitrous acid
Nitrous acid is oxidized to nitric acid and nitric oxide reoxidized to
NO2

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Chile Saltpetre method

Chile Saltpetre method is based on a laboratory scale reaction. It was once
popular in the 1920’s. Chile saltpeter, a material which contains sodium
nitrate NaNO3 with percentage around 35-60%, and remaining percentage
compounds with KNO3 and NaCl. Refined Chile Saltpetre and concentrated
sulfuric acid are mixed in the following chemical reaction to produce the
desired nitric acid in vapor form. The vapor is then condensed into liquid
nitric acid.
NaNO3 + H2SO4 NaHSO4 + HNO3

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22. STORAGE AND PRESERVATION:-
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Store nitric acid in the original container. Dilute solutions must be stored in
acid resistant bottles. Do not store nitric acid near materials with which it
might react.
HNO3 and others acid are store in Teflon coated plastic container.
It is stored in acid resistance bottles.
It is not store near the material which are most reactive.

23. HYDROCHLORIC ACID
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24. INTRODUCTION
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Hydrochloric acid is a clear, colorless, highly pungent solution of hydrogen chloride (HCl) in
water. It is a highly corrosive, strong mineral acid with many industrial uses. Hydrochloric acid
is found naturally in gastric acid.
About 20 million tons of hydrochloric acid are produced worldwide annually.
Hydrochloric acid (HCl) is listed as a Title III Hazardous Air Pollutant.
Hydrochloric acid is a versatile chemical used in a variety of chemical processes, including
hydrometallurgical processing (e. g., production of alumina and/or titanium dioxide), chlorine
dioxide synthesis, hydrogen production, activation of petroleum wells, and miscellaneous
cleaning/etching operations including metal cleaning (e. g., steel pickling).Also known as
muriatic acid

25. PROPERTIES
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Appearance:
Odor:
Boiling point:
Melting point:
Vapor pressure:
Density:
colorless, fuming liquid
pungent odor
3C (127F)
74C (-101F)
190 mm Hg @ 25C (77F)
1.18 (water = 1)

26. PREPARATION METHODS
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Synthesis from elements (Burning Process)
Organic By-product Synthesis.
Metallic chlorides with Sulfuric acid.
Waste Incineration.
Thermal decomposition of hydrated heavy metals
Hydrochloric acid may be manufactured by several different processes, although over 90
percent of the HCl produced in the world is a byproduct of the chlorination reaction.

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32. ORGANIC BY-PRODUCT SYNTHESIS
Hydrochloric acid is made during chlorination of
organicproducts as follows:
•RH2+ Cl2 → RCl + HCl
Hydrochloric acid is also made during fluorination of chlorinated organic
products to manufacture (hydro)chlorofluorocarbons as follows:
•RCl + HF → RF + HCl
Where RCl stands for chloroform, trichloro ethane, etc andRF
stands for (hydro) chlorofluorocarbons
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33. •As a byproduct of chlorination, e. g., in the production of dichloromethane,
trichloroethylene, perchloroethylene, or vinyl chloride:
•C2H4 Cl2 → C2H4Cl2
•C2H4Cl2 → C2H3Cl HCl
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34. FLOW SHEET
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Chlorination
Process
HCL
Absorption

Scrubber
HCL & Cl2
Chlorination Gases Vent Gas
Dilute HCL
Concentrated
HCL

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36. BY THERMAL DECOMPOSITION
By thermal decomposition of the hydrated heavy-metal chlorides from spent
pickle liquor in metal treatment: 2FeCl3 6H2O → Fe2O3 3H2O 6HCl

FROM INCINERATION
From incineration of chlorinated organic waste: C4H6Cl2 5O2 → 4CO2 2H2O
2HCl
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37. USES
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For pickling Steel
For the manufacturing of PVC pipes
For the production of compounds that used in wastewater treatment
For manufacturing of Dyes and Fertilizers
It is used in textile and rubber industries

38. HEALTH SAFETY & ENVIRONMENT
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Concentrated hydrochloric acid (fuming hydrochloric acid) forms acidic mists. Both the mist and
the solution have a corrosive effect on human tissue, with the potential to damage respiratory
organs, eyes, skin, and intestines irreversibly. Upon mixing hydrochloric acid with common
oxidizing chemicals, such as sodium hypochlorite (bleach, NaClO) or potassium
permanganate (KMnO4), the toxic gas chlorine is produced
NaClO + 2HCl → H2O + NaCl + Cl2
2KMnO4 + 16HCl → 2MnCl2 + 8H2O + 2KCl + 5Cl2
PbO2 + 4HCl → 2H2O + PbCl2 + Cl2

39. STORAGE AND PRESERVATION
Store in a cool, dry, ventilated storage area with acid resistant floors and good
drainage.
XLPE tanks are recommended but HDPE, LDPE, FRP, rubber-lined steel and
•polypropylene tanks can also store HCL.
The tanks use for storage of HCL its specific gravity should be 1.9
Employ fume scrubbers for HCL vapor mitigation.
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