1. Hydrochloric Acid
• Burner Process:
Chlorine and Hydrogen react to form Hydrogen Chloride
H2 + Cl2 2 HCl (+184 KJ)
The gases are passed through a burner nozzle
They are ignited inside a combustion chamber (chamber is made of graphite)
The chamber is cooled by water such that the HCl gas produced cools down and absorbed into water to
make HCl acid
https://www.youtube.com/watch?v=HJvn-rH_lLQ&ab_channel=IITKharagpurJuly2018
https://www.essentialchemicalindustry.org/chemicals/hydrogen-chloride.html
3. Use of HCl
• Metal Cleaning
• Pickling of Metals
• Manufacturing of metal chlorides
• Pb(NO3)2 + 2HCl PbCl2 + 2HNO3
• Neutralization in inorganic and organic
chemistry
• Hydrolysis of proteins and carbohydrates
• Manufacture glue
• Purify common salt
• Bleaching in textile industry
• Chemical reagent in laboratories
Laboratory preparations
• NaCl + H2SO4 NaHSO4 + HCl
• NaCl + NaHSO4 HCl + Na2SO4
4. Nitric Acid / Aqua fortis / Oxy-acid of Nitrogen
https://www.youtube.com/watch?v=rjuA6d8LL1w&ab_channel=COLLEGECHEMISTRY
OSTWALD’s Process:
Step 01: Oxidation of NH3 to NO
NH3 + excess air NO (Catalytic chamber (Pt) / Converter)
To ensure up to 95% of NH3 converts to NO:
• Temperature: 550 – 600C
• Pressure: 4 – 5 atm
• Excess of Oxygen
• Pt catalyst
NO is passed through chiller with temperature 150C
5. OSTWALD’s Process:
Step 02: Oxidation of NO to NO2 Step 03: Formation of HNO3
NO2 enters the absorption tower where NO2 is
absorbed by water
Laboratory preparation of nitric acid
KNO3 + H2SO4 KHSO4 + HNO3
NaNO3 + H2SO4 NaHSO4 HNO3