Lead Group 14 (IVa) of the periodic table contains lead (Pb), a soft, silvery-white, or grey metal. Lead is a poor conductor of electricity and is exceedingly malleable, ductile, and dense. It has an atomic number of 82.
Nitrate is a member of one of two classes of compounds derived from nitric acid. Nitrate is an ionic compound that contains ammonium nitrate with cations such as nitrate ion NO–3 and NH4+.
Lead nitrate is an inorganic substance of the chemical formula Pb (NO3)2. It usually occurs as a colorless crystal or white powder and, unlike most other lead (II) salts, is water-soluble. Since the Middle Ages, lead nitrate (II) has been produced in small quantities from metallic lead or lead oxide in nitric acid for direct use in the production of other lead compounds. In the 19th century, lead nitrate II formulations were first commercially produced in Europe and the United States. For lead paint pigments, it is used as raw material. The stability of polyester and nylon used in photothermography paper coatings is one of its many uses.
Structure of lead nitrate
Lead is a transition metal and nitrate is a non-metal category. Nitrate is a polyatomic ion. As a result, lead (II) nitrate is a fusion of metals and non-metals. (II) indicates that in lead (II) nitrate, lead has a charge of +2 and nitrate has a charge of -1. The formula for lead (II) nitrate is Pb (NO3)2, which uses a cross-shaped approach to neutralize the charge.
Preparation of Lead nitrate
- Lead nitrate is formed when lead(II) oxide reacts with strong nitric acid
PbO + 2 HNO3(con.) → Pb(NO3)2 ↓ + H2O
- It is also possible to vaporize the solution produced by reacting metallic lead with weak nitric acid.
Pb + 4 HNO3 → Pb(NO3)2 + 2 NO2 + 2 H2O
- Lead (II) nitrate solution and crystals result from the treatment of lead-bismuth waste from a lead refinery.
- Lead nitrate is produced when lead carbonate reacts with strong nitric acid. The reaction is as follows
PbCO3 + 2 HNO3 → Pb(NO3)2 + H2O + CO2
- Lead nitrate can be prepared when lead sulfide reacts with strong nitric acid, reaction as follows
3PbS +8HNO3 → 3Pb(NO3)2 + 3S +2NO + 4H2O
Physical properties
- Lead (ll) nitrate is a crystalline white solid that dissolves readily in water to form an almost transparent solution.
- At 0oCelsius, lead (ll) nitrate dissolves 376.5 grams per liter, 597 grams per liter at 25o Celsius, and 127 grams per liter at 100o Celsius.
- It has molar mass 331.2 g/mol.
- It is colorless or white in appearance.
- It is soluble in water.
- Melting point- decomposes.
- The density is 4.53 g/cm3.
- Ph level is 6.5.
- The temperature at which it melts is 470o Celsius.
Chemical Properties
- Lead (II) nitrate interacts with sodium hydroxide to form a white precipitate, lead (II) hydroxide.
Pb(NO3)2 + 2NaOH → Pb(OH)2 + 2NaNO3
First, a precipitate of lead (II) hydroxide is formed, which is dissolved by excess sodium hydroxide and is called sodium plum. Form a colorless solution.
- The reaction of lead (II) nitrate with a potassium iodide solution produces a bright yellow precipitate of lead iodide
Pb(NO3)2 + 2KI → PbI2 + 2KNO3
This is usually shown using a conventional golden rain experiment in which lead iodide is dissolved in boiling water and crystallizes to a beautiful golden color when cooled.
- Lead (II) nitrate reacts with potassium chromate to form a yellow precipitate, lead (II) chromate.
Pb(NO3)2 + K2CrO4 → 2KNO3 + PbCrO4
- Lead (II) nitrate also undergoes a substitution reaction with ammonium sulfate to form a white precipitate, lead sulfate.
Pb(NO3)2 + (NH4)2S → PbS + NH4NO3
-
Lead (ll) nitrate thermal decomposition
While holding the test tube diagonally, 1 g of lead nitrate (II) is placed in the test tube on the flame of the Bunsen burner. Heat with. position. After a while, you will hear the familiar popping sound, followed by the release of brown gas.
2Pb(NO3)2 → 2PbO + 4NO2 + O2
Pyrolysis of lead (II) nitrate produces lead oxide, nitrogen dioxide (brown gas), and oxygen gas.
Uses of Lead (II) Nitrate
- Matches and special explosives include lead nitrate (II).
- Lead (II) nitrate is also used in the dye and photography industry.
- Lead (II) nitrate is also used for engraving.
- Lead (II) nitrate can also be used to support the leaching process in the cyanidation process.
Sample Problems
Question 1: What is the process of removing lead nitrate from water?
Solution:
Ion exchange, distillation, and reverse osmosis are all effective methods for removing nitrate from water. Contact your local health department for further information. It is impossible to eliminate nitrate from water by heating or boiling it.
Question 2: What is the chemical formula for lead nitrate solution?
Solution:
The chemical formula for lead (II) nitrate is Pb(NO3)2. The molar mass is 331.2 g/mol. The molecule is made up of one lead cation Pb2+ and two nitrate anions NO3-. With the lead cation, the two anions create an ionic connection.
Question 3: Give observations on heating lead nitrate crystals in a hard glass tube.
Solution:
2Pb(NO3)3 → 2PbO + 4NO2 + O2
When lead nitrate crystals are heated, lead oxide is produced, which is yellow in color, and nitrogen dioxide, which is reddish-brown in color, is emitted.
Question 4: Give a reaction in which one of the products is lead iodide.
Solution:
When lead nitrate (aqueous) is combined with potassium iodide, the iodide ion displaces nitrate from lead nitrate, and nitrate reacts with potassium to generate potassium nitrate, while lead reacts with iodine to form lead iodide. As a result, two chemicals are formed: lead iodide, a yellow solid, and potassium nitrate.
Pb(NO3)2 (aq) + 2KI (aq) →PbI2 (s) + 2KNO3 (aq)
(yellow solid)
Question 5: When lead nitrate is heated to a high temperature, what is the result?
Solution:
2Pb(NO3)2 → 2PbO + 4NO2 + O2
The reaction described above is a decomposition reaction in which lead (ll) nitrate is degraded. When lead nitrate is heated to a high temperature, it decomposes into lead oxide, nitrogen oxide, and oxygen. This reaction can also be used to produce nitrogen dioxide gas and can be used as a rodenticide.
Question 6: For the following, make one meaningful observation: The excess lead nitrate solution is neutralized with sodium hydroxide solution drop by drop till the excess is reached.
Solution:
Pb(NO3)2 + 2NaOH → Pb(OH)2 + 2NaNO3
The lead hydroxide forms a white precipitate when sodium hydroxide is added drop by drop, and when sodium hydroxide is added in excess, the white precipitate dissolves.
Pb(OH)2 + 2NaOH → NaPbO2 + 2H2O
(excess) (sodium plumbite)