Yes, HNO3 (nitric acid) is a strong electrolyte. When dissolved in water, it completely ionizes into hydrogen ions (H+) and nitrate ions (NO3)-, resulting in a high concentration of ions in the solution. This makes it an effective conductor of electricity.
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Key Takeaways: Is HNO3 a Strong Electrolyte?
- HNO3 (nitric acid) is a strong electrolyte because it completely dissociates into ions (H+ and NO3–) when dissolved in water, making it an efficient conductor of electricity.
- The degree of dissociation of HNO3 is much higher compared to weak electrolytes, which only undergo partial dissociation, leaving some molecules unchanged in solution.
- HNO3 is used as an electrolyte in various applications, such as metal etching, fertilizer production, explosives manufacturing, laboratory procedures, pickling, cleaning, and rocket propellants.
Why is HNO3 a strong electrolyte?
HNO3, or nitric acid, is a strong electrolyte due to its ability to completely dissociate into ions when dissolved in water. Strong electrolytes are substances that dissociate into ions to a high extent, while weak electrolytes only partially dissociate. 1
In the case of HNO3, when it is dissolved in water, the following reaction occurs:
HNO3 (aq) → H+ (aq) + NO3– (aq)
As you can see, HNO3 breaks apart into hydrogen ions (H+) and nitrate ions (NO3-) in solution. These ions are electrically charged and can conduct electricity by facilitating the movement of charge-carrying particles.
The strong dissociation of HNO3 into ions is a result of its molecular structure and the nature of its chemical bonds. Nitric acid has a highly polar covalent bond between hydrogen and nitrogen, making the hydrogen atom partially positive and the nitrate ion partially negative. This polarity allows for the easy separation of H+ and NO3- ions when dissolved in water.
In contrast, weak electrolytes only partially dissociate into ions, and some of the original molecules remain intact in solution. This is typically due to weaker chemical bonds or less polar molecules.
In summary, HNO3 is a strong electrolyte because it dissociates almost completely into ions when dissolved in water, allowing it to conduct electricity effectively.
Degree of dissociation of HNO3 compared to a weak electrolytes
The degree of dissociation of HNO3 is much higher compared to weak electrolytes. HNO3 is a strong electrolyte, meaning it almost completely dissociates into ions when dissolved in water. In contrast, weak electrolytes only undergo partial dissociation, with a significant portion of the original molecules remaining intact in solution.
The degree of dissociation refers to the extent to which a substance breaks down into ions when dissolved in a solvent, typically water. 2 As mentioned earlier, HNO3 is a strong electrolyte and undergoes almost complete dissociation into ions:
HNO3 (aq) → H+ (aq) + NO3– (aq)
On the other hand, weak electrolytes only undergo partial dissociation. For example, a weak acid like acetic acid (CH3COOH) partially dissociates into ions when dissolved in water:
CH3COOH (aq) ⇌ H+ (aq) + CH3COO– (aq)
In this case, not all acetic acid molecules dissociate into ions; some remain as intact molecules. This is due to weaker chemical bonds or less polar molecular structures in weak electrolytes.
In summary, the degree of dissociation of HNO3 is significantly higher compared to weak electrolytes because HNO3 almost fully dissociates into ions when dissolved in water, while weak electrolytes only undergo partial dissociation, leaving a substantial portion of the molecules unchanged.
Applications in which HNO3 is used as an electrolyte
HNO3, or nitric acid, is used as an electrolyte in various industrial and laboratory applications. Some of the common applications include:
- Etching and metal finishing: Nitric acid is utilized in metal etching and metal finishing processes. 3 It can be employed to remove oxides and impurities from metal surfaces, providing a clean and smooth finish. This is particularly important in the manufacturing of electronic components and microchips.
- Manufacture of fertilizers: Nitric acid is a key component in the production of ammonium nitrate, a widely used nitrogen-based fertilizer. 4 5 It is used to neutralize ammonia gas and create ammonium nitrate, an essential nutrient for plants’ growth.
- Explosives production: Nitric acid is a crucial ingredient in the manufacturing of explosives, such as trinitrotoluene (TNT) and nitroglycerin. 6 It is used in the nitration process to introduce nitro groups into organic compounds, thereby increasing their explosiveness.
- Laboratory applications: In laboratories, dilute nitric acid is commonly used for various purposes, such as testing for the presence of metals, cleaning glassware, etching, making synthetic fibers and preparing solutions for chemical analysis. 7
- Pickling and cleaning: Nitric acid is used in pickling processes to remove rust and scale from metal surfaces. 8 9 It is also employed in cleaning applications to remove stubborn stains and contaminants from equipment and surfaces.
- Rocket propellants: Nitric acid, along with other oxidizers, is used in the formulation of rocket propellants for aerospace applications. 10
It’s important to note that while nitric acid has various industrial uses, it is a strong acid and should be handled with caution due to its corrosive and hazardous nature. Safety precautions and proper handling procedures are essential when working with this chemical.
Further reading
Why is NaCl (Sodium Chloride) a Strong Electrolyte?
Why is KCl a Strong Electrolyte?
Is Sucrose an Electrolyte?
Is Glucose (C6H12O6) an Electrolyte?
Is CH3OH (Methanol) an Electrolyte?
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References
- Stolaf.edu https://www.stolaf.edu/depts/chemistry/courses/toolkits/121/js/naming/elec.htm
- Dissociation (chemistry) – Wikipedia. (2014, June 1). Dissociation (Chemistry) – Wikipedia. https://en.wikipedia.org/wiki/Dissociation_(chemistry)
- Speight, J. G. (2022). Chemical products. Biomass Processes and Chemicals, 293–353. https://doi.org/10.1016/b978-0-12-821679-8.00007-7
- Sharma, C., Singh, R., Gurjar, B., Sahu, V., & Bhattacharya, S. (2017). Emissions of Reactive Nitrogen From Energy and Industry Sectors in India. The Indian Nitrogen Assessment, 483–488. https://doi.org/10.1016/b978-0-12-811836-8.00030-6
- Ammonium nitrate – Wikipedia. (2015, March 13). Ammonium Nitrate – Wikipedia. https://en.wikipedia.org/wiki/Ammonium_nitrate
- Nitric Acid – Molecule of the Month – November 2007 – HTML only version. (n.d.). Nitric Acid – Molecule of the Month – November 2007 – HTML Only Version. https://www.chm.bris.ac.uk/motm/nitric/nitrich.htm
- Nitric acid – DCCEEW. (2022, June 30). Nitric Acid – DCCEEW. https://www.dcceew.gov.au/environment/protection/npi/substances/fact-sheets/nitric-acid
- Pickling and Passivation of Stainless Steel. (n.d.). Blog. https://www.assda.asn.au/blog/304-pickling-and-passivation-of-stainless-steel
- Worldstainless.org https://www.worldstainless.org/Files/issf/non-image-files/PDF/Euro_Inox/Passivating_Pickling_EN.pdf
- Nasa.gov https://history.nasa.gov/conghand/propelnt.htm