What is Zinc Nitrate Formula Properties Reactions and Uses in Chemistry
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
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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 Structure Preparation and Chemical Behavior
1. What is zinc nitrate?
Zinc nitrate is an inorganic salt with the chemical formula Zn(NO3)2 composed of zinc ions and nitrate ions. It consists of one Zn2+ cation and two NO3- anions.
- Commonly found as the hexahydrate: Zn(NO3)2·6H2O.
- It is a colorless, crystalline, and highly soluble compound.
- Used in laboratories, fertilizers, and as a precursor in zinc oxide preparation.
2. What is the formula and molar mass of zinc nitrate?
The chemical formula of zinc nitrate is Zn(NO3)2 and its molar mass is approximately 189.4 g·mol-1 (anhydrous form).
- Zn = 65.38 g·mol-1
- 2 × (N = 14.01 g·mol-1 + 3 × O = 16.00 g·mol-1)
- For the hexahydrate, Zn(NO3)2·6H2O, molar mass ≈ 297.5 g·mol-1.
3. How is zinc nitrate prepared in the laboratory?
Zinc nitrate is prepared by reacting zinc metal or zinc oxide with nitric acid to form Zn(NO3)2 and water (and nitrogen oxides if metal is used).
- From zinc oxide: ZnO(s) + 2HNO3(aq) → Zn(NO3)2(aq) + H2O(l)
- From zinc metal (with dilute acid): 3Zn(s) + 8HNO3(aq) → 3Zn(NO3)2(aq) + 2NO(g) + 4H2O(l)
- The solution is evaporated to obtain crystals.
4. Is zinc nitrate soluble in water?
Yes, zinc nitrate is highly soluble in water because all nitrate salts are soluble. When dissolved, it dissociates as:
- Zn(NO3)2(aq) → Zn2+(aq) + 2NO3-(aq)
5. What happens when zinc nitrate is heated?
When heated, zinc nitrate decomposes to form zinc oxide, nitrogen dioxide, and oxygen gas. The balanced thermal decomposition reaction is:
- 2Zn(NO3)2(s) → 2ZnO(s) + 4NO2(g) + O2(g)
6. What type of compound is zinc nitrate?
Zinc nitrate is an ionic compound composed of metal cations and polyatomic anions. It contains:
- Zn2+ (a metal ion)
- NO3- (a polyatomic nitrate ion)
7. What are the common uses of zinc nitrate?
Zinc nitrate is mainly used as a precursor for zinc oxide and in chemical synthesis. Key applications include:
- Preparation of ZnO by thermal decomposition.
- Manufacture of dyes and mordants in textile processing.
- Laboratory reagent in inorganic chemistry.
- Component in some fertilizers as a zinc micronutrient source.
8. Is zinc nitrate acidic or basic in solution?
Zinc nitrate solution is slightly acidic due to hydrolysis of the zinc ion in water. The Zn2+ ion reacts weakly with water to produce hydrogen ions:
- Zn2+(aq) + H2O(l) ⇌ ZnOH+(aq) + H+(aq)
9. What is the difference between zinc nitrate and zinc nitrite?
The key difference is that zinc nitrate contains the nitrate ion (NO3-) while zinc nitrite contains the nitrite ion (NO2-).
- Zinc nitrate formula: Zn(NO3)2
- Zinc nitrite formula: Zn(NO2)2
- Nitrate has three oxygen atoms; nitrite has two.
- Zinc nitrite is less stable and more reactive compared to zinc nitrate.
10. How do you calculate the percentage composition of zinc in zinc nitrate?
The percentage of zinc in Zn(NO3)2 is calculated using its molar mass and is approximately 34.5%. Steps:
- Molar mass of Zn(NO3)2 ≈ 189.4 g·mol-1
- Atomic mass of Zn = 65.38 g·mol-1
- Percentage of Zn = (65.38 ÷ 189.4) × 100 ≈ 34.5%
