The document discusses the production and properties of nitric acid and hydrochloric acid. It describes the main industrial processes for manufacturing each acid, including the Ostwald process for nitric acid production and electrolysis of sodium chloride to produce chlorine for hydrochloric acid synthesis. Key safety considerations for acid storage are outlined, emphasizing the need for corrosion-resistant materials and segregation of different acid types.

1. T
H
M ZARYAB
WALEED
B1F17BSCHOO95

2. Topics
Raw materials, flow sheet diagram Unit operations and
unit processes of Nitric Acid And Hydrochloric acid..
HCL, HNO3,

3. Nitric acid
 Nitric acid, (HNO3),
 Colourless,
 Fuming, and
 Highly corrosive liquid

4. PROPERT
IES
• FORMULA: HNO3
• IUPAC ID: NITRIC ACID
• MOLAR MASS: 63.01
G/MOL • BOILING POINT: 83
°C
• DENSITY: 1.51 G/CM³
• MELTING POINT: -42 °C

5. • CORROSIVE
• A CORROSIVE SUBSTANCE IS DEFINED AS A MATERIAL CAPABLE OF DAMAGING OR
DESTROYING OTHER SUBSTANCES ON CONTACT VIA A CHEMICAL REACTION.
EXAMPLES OF CORROSIVE CHEMICALS INCLUDE ACIDS, OXIDIZERS, AND BASES.
SPECIFIC EXAMPLES INCLUDE SODIUM HYDROXIDE, NITRIC ACID, AND HYDROGEN
PEROXIDE.
• A CHEMICAL THAT CAUSES VISIBLE DESTRUCTION OF, OR IRREVERSIBLE
ALTERATIONS IN, LIVING TISSUE BY CHEMICAL ACTION AT THE SITE OF CONTACT.
• AS CORROSIVE SUBSTANCES CAN DEGRADE CERTAIN MATERIAL SUCH AS METAL
AND STONE, IT MEANS THAT THEY HAVE A VERY STRONG ABILITY TO BREAK DOWN
AND DESTROY HUMAN TISSUE. WHEN CORROSIVE MATERIALS TOUCH YOUR SKIN,
THEY WILL IMMEDIATELY START TO DISSOLVE YOUR FLESH, LEAVING BURNS. IF
CORROSIVE SUBSTANCES COME IN CONTACT WITH YOUR EYES, THEY CAN HAVE
VERY SEVERE EFFECTS SUCH AS; DAMAGING THE CORNEA AND EVEN CAUSING
BLINDNESS.

6. MANUFACTUR
ES
METHOD
1
Single displacement synthesis.
2
Ostwald process.
3
Birkeland and Eyde process or arc
process

7. Single displacement synthesis./ Laboratory
preparation

8. O
BIRKELAND AND EYDE PROCESS OR ARC
PROCESS • 1. PRINCIPLE :
• N2 AND O2 IS PRESENT IN THE AIR ARE USED FOR THE MANUFACTURE OF NITRIC
ACID.
• N2 + O2 ——-> 2NO – 43.2 K.CALORIE
• THERE IS NO EFFECT OF PRESSURE ON THE REACTION BECAUSE THERE IS NO
CHANGE IN VOLUME. THE TEMPERATURE FOR THE REACTION IS 3000 C. NO IS
OXIDIZED TO NO2 (NITROGEN DIOXIDE) WHICH ON DISSOLVING IN WATER GIVES
HNO3.
• 2NO + O2 ——-> 2NO2
• 3NO2 + H2O —–> 2HNO3 + NO

9. RAW
MATERIALS
• A m m o n i a
• W a t e r
• A i r
• C a t a l y s t ( p l a t i n u m -
r h o d i u m g a s )

10. STEPS INTHE PRODUCTION
O x i d a t i o n o f
a m m o n i a N H 3
O x i d a t i o n o f
n i t r i c o x i d e
A b s o r p t i o n o f
N O 2

11. MANUFACTURING OF NITRIC ACID BY OSTWALD
PROCESS • THE OSTWALD PROCESS CONVERTS AMMONIA TO NITRIC ACID
• IN STEP 1, AMMONIA IS OXIDIZED TO FORM NITRIC OXIDE AND ALSO NITROGEN
DIOXIDE.
• THEN IN STEP 2, THE NITROGEN DIOXIDE THAT WAS FORMED IS ABSORBED IN
WATER. THIS IN- TURN FORMS NITRIC ACID.

13. STEP
1
FORMATION OF NITRIC
ACID• OXIDATION OF AMMONIA IS CARRIED OUT IN A CATALYST CHAMBER IN WHICH
ONE PART OF AMMONIA AND EIGHT PARTS OF OXYGEN BY VOLUME ARE
INTRODUCED.
• THE TEMPERATURE OF CHAMBER IS ABOUT 600OC.
• THIS CHAMBER CONTAINS A PLATINUM GAUZE WHICH SERVES AS CATALYST.
• 4NH3 + 5O2 ↔ 4NO + 6H2O ?H -24.8 KCAL/MOL

14. STEP 2 — 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 A HEAT EXCHANGER WHERE THE TEMPERATURE OF
NITRIC OXIDE IS REDUCES TO 150OC. NITRIC OXIDE AFTER COOLING IS
TRANSFERRED TO ANOTHER OXIDIZING TOWER WHERE AT ABOUT 50OC IT IS
OXIDIZED TO NITROGEN DIOXIDE (NO2).
• 2NO + O2 ↔2 NO2

15. STEP 3 — FORMATION OF HNO3
• NITROGEN DIOXIDE FROM SECONDARY OXIDATION CHAMBER IS INTRODUCED
INTO A SPECIAL ABSORPTION TOWER.
• NO2 GAS PASSED THROUGH THE TOWER AND WATER IS SHOWERED
OVER IT. BY THE ABSORPTION, NITRIC ACID IS OBTAINED.
• 3NO2 + H2O -> 2HNO3 + NO

16. STEP 4 — CONCENTRATION
• IN ORDER TO INCREASE THE CONCENTRATION OF HNO3, VAPORS OF HNO3 ARE
PASSED OVER CONCENTRATED H2SO4.
• BEING A DEHYDRATING AGENT, H2SO4 ABSORBS WATER FROM HNO3 AND
CONCENTRATED HNO3 IS OBTAINED.

18. INDUSTRIAL USES
• E x p l o s i v e s e . g T N T , N i t r o -
g l y c e r i n , G u n c o t t o n , A m m o n a l
•
F e r t i l i z e r s s u c h a s c a l c i u m n i t r a t e , a m m o n i u
m n i t r a t e
• D y e s , p e r f u m e s , D r u g s
• S y n t h e t i c f i b e r s s u c h a s N y l o n
•
F o r s u l p h u r i c a c i d p r o d u c t i o n f r o m n i t r i c a c i d
b y t h e l e a d c h a m b e r p r o c e s s •
I n p u r i f i c a t i o n o f s i l v e r , g o l d , p l a t i n u m
•
F o r c a r v i n g d e s i g n s o n c o p p e r , b r a s s , b r o n z e

19. INTRODUCTION
• HYDROCHLORIC ACID IS A COLOURLESS AND ODOURLESS SOLUTION OF
HYDROGEN CHLORIDE AND WATER; WITH CHEMICAL FORMULA HCL. ONCE
COMMONLY REFERRED TO AS MURIATIC ACID OR SPIRIT OF SALT, THIS ACID IS A
HIGHLY CORROSIVE CHEMICAL COMPOUND WITH SEVERAL APPLICATIONS IN
INDUSTRY.

20. HCL
APPLICATION
• USED IN MANUFACTOR OF ORGANIC ACID
• HCL AS CLEANING AGENT
• USED TO NEUTRALIZE
• USED TO REGULATE PH LEVEL

21. CH4+CL2=
CH3CL+HCL
H2S + CL2 = S +
HCL
HCL AS
BY
Product
formatio
n
2H2
O
+ 2CL2
=
4
HCL
PCL3+ 3H2O = H3PO3
+
HCL

22. RAW
MATETAIL
NaCl
salt
Water
Electricit
y

23. PREPARATION OF HCL DIRECT SYNTHESIS

Brine (mixture of sodium chloride and water) solution is electrolyzed producing chlorine (Cl2),
sodium hydroxide, and hydrogen (H2).
 The pure chlorine gas can be combined with hydrogen to produce hydrogen chloride.Cl2(g) + H2(g) →
2 HCl(g)

24. PREPARATION OF HCL LABORATORY METHOD
 It is prepared industrially by the combustion of
Hydrogen,
 H2, in Chlorine, Cl2.H2 + Cl HCl
 ii) Hydrogen Chloride may be prepared in the laboratory by heating Concentrated SulphuricAcid, with
Sodium Chloride.
 NaCl + H2SO4 → NaHSO4 + HCl
 This reaction occurs at room temperature. Provided there is salt remaining in the generator and it is
heated above 200 degrees Celsius, the reaction proceeds to
 NaCl + NaHSO4 → HCl + Na2SO4

25.  iii) The chlorides of non-metals (e.g. Phosphorus trichloride, PCl3) are covalent compounds. These
chlorides fume in air and are readily hydrolysed to yield either an acid or an acidic oxide.
 For example, Phosphorus trioxide, reacts with the Moisture, in air to form PhosphorousAcid, and
Hydrogen Chloride.
 PCl3 + 3H2O H3PO3 + 3HClPhosphorus pentachloride, is hydrolysed by hot water, to give
Orthophosphorus Acid, (i.e. Phosphoric(V)Acid) and Hydrogen Chloride.
 PCl5 + 4H2O H3PO4 + 5HClPhosphorus pentachloride, is also hydrolysed by cold Water,to give
Phosphorus oxychloride.
 PCl5 + H2O → POCl3 + 2 HCl

28. ACID STORAGE
• MINERAL ACIDS, INCLUDING PHOSPHORIC, HYDROCHLORIC, NITRIC, SULFURIC, AND PERCHLORIC
ACID CAN BE STORED IN A CABINET DESIGNED FOR CORROSIVE ACIDS. NITRIC ACID CAN ALSO BE
STORED WITH OXIDIZERS. THESE NON- METALLIC CABINETS HAVE NO INTERNAL METALLIC PARTS,
ACID RESISTANT COATING AND A CABINET FLOOR CONSTRUCTED TO BE ABLE TO CONTAIN
SPILLAGE. VOLATILE ACIDS, SUCH AS OLEUM OR FUMING NITRIC ACID, SHOULD BE STORED EITHER
IN AN ACID CABINET OR IN A VENTED CABINET, SUCH AS THE FUME HOOD BASE, PARTICULARLY
AFTER THEY HAVE BEEN OPENED. CONCENTRATED MINERAL ACIDS CAN BE VERY REACTIVE,
EVEN WITH EACH OTHER.
• ORGANIC ACIDS SUCH AS ACETIC ACID SHOULD BE STORED SEPARATELY FROM MINERAL ACIDS.
WHILE IT IS ALWAYS BEST TO SEGREGATE, ACETIC ACID CAN BE STORED OTHER FLAMMABLE
LIQUIDS.
• PICRIC ACID CAN FORM EXPLOSIVE SALTS WITH MANY METALS, OR BY ITSELF WHEN DRY. IT IS
INCOMPATIBLE WITH OTHER STORAGE GROUPS AND SHOULD BE STORED SEPERATELY.
PERCHLORIC ACID IS AN EXTREMELY POWERFUL OXIDIZER AND MUST BE KEPT AWAY FROM ALL
ORGANIC MATERIALS. IT SHOULD ALSO BE STORED SEPERATELY.

30. • IF YOU ARE STORING STRONG ACIDS SUCH AS HYDROCHLORIC ACID AND SULFURIC ACID, IT
IS BETTER TO USE A CABINET THAT IS CONSTRUCTED FROM A CORROSIVE RESISTANT
MATERIAL SUCH AS POLYETHYLENE. IF YOU
ARE STORING WEAKER ACIDS, THEY CAN BE SAFELY STORED IN A METAL CABINET THAT HAS A
CORROSIVE RESISTANT LINING
• STORAGE: HYDROCHLORIC ACID SHOULD BE KEPT IN A TIGHTLY CLOSED CONTAINER AND
STORED IN CHEMICAL AREA THAT IS COMPATIBLE WITH OTHER CHEMICALS. STORE IN A
SECURE, WELL-VENTILATED AREA, THAT IS WELL MARKED, AND AWAY FROM THE GENERAL
WORK POPULATION. DO NOT STORE NEAR OXIDIZING MATERIALS.
• TYPES OF CONTAINERS: THE SHIPPING CONTAINERS USED FOR HYDROCHLORIC ACID ARE
THOSE RAIL TANKS BE TIGHTLY SEALED, SUCH AS ACID-RESISTANT BOTTLES (INCLUDING
POLYETHYLENE CONTAINERS, ETC.), AND STEEL DRUMS TANK TRUCKS, TANK CARS, AND
TANKERS WITH CORROSION RESISTANT LININGS
• IF YOU KEEP READING THE MANUAL THERE IS VALUABLE INFORMATION ABOUT HANDLING,
TRANSPORTATION, AND RULES TO KEEP THE HUMAN SAFETY.

31. • ORIGINALLY POSTED BY ENGAGER
HIGHLY CONCENTRATED OR ANHYDROUS NITRIC ACID IS UNSTABLE AND DECOMPOSES SLOWLY
UNDER ORDINARY CONDITIONS, SEALS MUST NOT BE TIGHT BECAUSE DECOMPOSITION
PRODUCTS WILL GENERATE PRESSURE AND BOTTLE WILL FINALY CRACK AND SPILL ACID ALL
AROUND. HOWEVER THIS ACID CAN BE SAFELY STORED IN GLASS CONTAINER WITH TIGHT GLASS
LID IN DEEP FREEZE SECTION OF HOME REFRIGIRATOR. DECOMPOSITION IS SLOWED GREATLY AT
THIS CONDITIONS, AND NO2 GAS CANNOT GENERATE PRESSURE BECAUSE IT LIQUIFIES AT THIS
TEMPS. LIQUID NO2 REACTS WITH WATER CONTAMINANTS IN ACID TO FORM MORE NITRIC ACID,
SO SOME KIND OF CONSTANT EQUILIBRIUM EXIST. I STORED CONCENTRATED HNO3 IN THIS WAY
FOR MORE THEN 2 YEARS WITHOUT ANY PROBLEMS AND DEGREE OF DECOMPOSITION WAS LOW
(VERY SLIGHT YELLOW COLOR).
70% NITRIC ACID AND BELOW CAN BE STORED FOREVER IN DARK GLASS BOTTLES WITH PLASTIC
LID, WITHOUT ANY DECOMPOSITION AT ORDINARY TEMPERATURE.
[EDITED ON 15-7-2008 BY ENGAGER]