How Is Zinc Nitrate Produced? Step-by-Step Guide and Uses
Zinc nitrate is an inorganic chemical compound that is a colorless crystalline solid with the chemical formula Zn(NO3)2. It is non-combustible but accelerates the burning of combustible materials. This white, crystalline salt is highly deliquescent (Deliquescent: Certain substances have the property to absorb moisture when exposed to the atmosphere at ordinary temperature, they initially become wet, lose their crystalline form and finally dissolve in water to form a saturated solution) in nature. Zinc nitrate solution is soluble in both water and alcohol. Nitrate compounds are mostly soluble in water. Nitrate materials are also good oxidizing agents. When they are mixed with hydrocarbons, these compounds can form a flammable mixture. Let’s discuss the Properties of Zinc nitrate, Zinc nitrate structure, and its uses.
Production of Zinc nitrate
Zinc nitrate is produced by dissolving zinc in a nitric acid solution. Below is the reaction with dilute and concentrated Nitric acid.
Zn + 2 HNO3 (diluted) → Zn(NO3)2 + H2
4 Zn + 10 HNO3 (concentrated) → 4 Zn(NO3)2 + NH4NO3 + 3H2O
After thermal decomposition of Zinc nitrate, it forms zinc oxide, oxygen, and nitrogen dioxide.
2 Zn(NO3)2 + Heat → 2ZnO + 4 NO2 + O2
Properties of Zinc nitrate
Zinc Nitrate Structure
(Image will be Uploaded Soon)
Uses of Zinc Nitrate
Zinc Nitrate is used as a catalyst in the manufacture of many chemicals, in the manufacturing of medicines, and dyes as a mordant.
It is used as a strong oxidizing agent.
It is used in liquid fertilizers.
It is also used as a latex coagulant.
Did You Know?
Zinc is a valuable catalytic agent in hydroxylation and other enzymatic reactions since it is an effective Lewis acid. The metal also has a versatile coordination geometry, allowing proteins to change conformations quickly to conduct biological reactions. Carbonic anhydrase and carboxypeptidase are two zinc-containing enzymes that are important for the regulation of carbon dioxide (CO2) and the digestion of proteins, respectively
Carbonic anhydrase converts CO2 into bicarbonate in vertebrate blood, and the same enzyme then converts bicarbonate back to CO2 for exhalation through the lungs. This conversion would take a million times longer without this enzyme at a standard blood pH of 7 or would require a pH of 10 or higher. Plants need the non-related -carbonic anhydrase for leaf formation, indole acetic acid (auxin) synthesis, and alcoholic fermentation.
Zinc is a trace element that is needed by humans, other mammals, plants, and microorganisms. Zinc is stored and transferred in metallothioneins, which are necessary for the function of over 300 enzymes and 1000 transcription factors. After iron, it is the second most common trace metal in humans, and it is the only metal found in all enzyme groups.
FAQs on Zinc Nitrate Explained: Key Concepts & Applications
1. What is zinc nitrate and what is its chemical formula?
Zinc nitrate is an inorganic chemical salt formed from zinc and the nitrate ion. It is a crystalline solid that is highly soluble in water. The correct chemical formula for zinc nitrate is Zn(NO₃)₂. It is commonly found in its hydrated form, zinc nitrate hexahydrate, with the formula Zn(NO₃)₂·6H₂O.
2. Why is an aqueous solution of zinc nitrate considered acidic?
An aqueous solution of zinc nitrate is acidic due to a process called salt hydrolysis. Zinc nitrate is a salt derived from a strong acid (Nitric Acid, HNO₃) and a weak base (Zinc Hydroxide, Zn(OH)₂). When dissolved in water, the zinc ion (Zn²⁺) reacts with water molecules, releasing hydrogen ions (H⁺) and making the solution acidic. The reaction is: Zn²⁺ + 2H₂O ⇌ Zn(OH)₂ + 2H⁺.
3. What are the products when solid zinc nitrate is heated strongly?
When solid zinc nitrate is heated, it undergoes thermal decomposition. This process breaks the compound down into three different products: a solid yellow residue (which cools to white) of zinc oxide (ZnO), a reddish-brown gas called nitrogen dioxide (NO₂), and colourless oxygen gas (O₂). The balanced chemical equation for this reaction is: 2Zn(NO₃)₂(s) → 2ZnO(s) + 4NO₂(g) + O₂(g).
4. What happens in the reaction between zinc metal and a copper(II) nitrate solution?
When zinc metal is placed in a blue solution of copper(II) nitrate, a single displacement reaction occurs. Zinc, being more reactive than copper, displaces the copper ions from the solution. This results in the formation of a colourless zinc nitrate solution and a reddish-brown solid deposit of copper metal. The characteristic blue colour of the copper solution gradually fades as the reaction proceeds. The equation is: Zn(s) + Cu(NO₃)₂(aq) → Zn(NO₃)₂(aq) + Cu(s).
5. Why can zinc displace copper from its salt solution, but copper cannot displace zinc?
This is explained by the electrochemical or reactivity series of metals. Zinc is positioned higher than copper in this series, which means it is more reactive and has a greater tendency to lose electrons (get oxidised). Because of its higher reactivity, zinc can readily displace the less reactive copper from its salt solution. Conversely, copper is less reactive and cannot displace the more reactive zinc from a zinc nitrate solution.
6. What is the importance of zinc nitrate hexahydrate?
Zinc nitrate hexahydrate (Zn(NO₃)₂·6H₂O) is the most common form of zinc nitrate. The six water molecules, known as water of hydration, are integrated into the crystal structure. This hydrated form is stable at room temperature and is the standard reagent used in laboratories for reactions involving zinc nitrate. Its presence is crucial for determining the correct molar mass for stoichiometric calculations.
7. How can zinc nitrate be prepared in a laboratory?
Zinc nitrate can be synthesised in a laboratory through several common reactions. A typical method involves reacting a zinc-based substance with nitric acid. The most common methods include:
- Reacting zinc metal with dilute nitric acid.
- Reacting zinc oxide (ZnO) with nitric acid.
- Reacting zinc carbonate (ZnCO₃) with nitric acid.
8. What are some key applications or uses of zinc nitrate?
Zinc nitrate has several important applications in various fields. Its primary uses include:
- As a mordant in the dyeing industry to help fix dyes to fabrics.
- As a catalyst in the synthesis of other chemical compounds.
- In laboratories as a source of zinc and nitrate ions for chemical reactions.
- In some medical preparations as an astringent and antiseptic agent.
