Acetic acid (CH3COOH) is a weak acid. 1 When dissolved in water, it only partially dissociates into its ions, releasing a limited amount of hydrogen ions (H+). This results in a lower concentration of H+ ions compared to strong acids, such as hydrochloric acid or sulfuric acid, which fully dissociate in water.
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Key Takeaways: Is Acetic Acid a Strong or Weak Acid?
- Acetic acid (CH3COOH) is a weak acid because it only partially dissociates in water, resulting in a limited release of hydrogen ions (H+).
- In contrast, strong acids like hydrochloric acid (HCl) fully dissociate, leading to a higher concentration of H+ ions and a stronger acidic effect.
- Acetic acid’s mild acidity finds application as a food preservative, household cleaner, pH adjuster in cosmetics, and catalyst in chemical synthesis.
Why is acetic acid a weak acid?
Acetic acid is a weak acid because it only partially dissociates in water, releasing a limited number of hydrogen ions (H+). This results in a relatively low concentration of H+ ions in the solution, leading to a weak acidic behavior compared to strong acids that fully ionize.
Acids are substances that can donate protons (H+) in aqueous solutions. 2 When acetic acid (CH3COOH) dissolves in water, it undergoes a partial dissociation, meaning only a fraction of the acetic acid molecules release their hydrogen ions.
The chemical equilibrium between the undissociated acid and its ions lies predominantly with the undissociated form. This limited ionization results in a relatively low concentration of H+ ions, leading to a weak acidic effect.
On the other hand, strong acids, like hydrochloric acid (HCl) or sulfuric acid (H2SO4), completely dissociate in water, releasing a large number of H+ ions, leading to a higher concentration of H+ ions in the solution and exhibiting a stronger acidic behavior. 3
Factors affecting the strength of an acid include the stability of the conjugate base (in this case, acetate ion, CH3COO-) and the strength of the bond between the hydrogen ion and the rest of the molecule.
In the case of acetic acid, the relatively stable acetate ion and the relatively strong bond between hydrogen and the acetate group contribute to its classification as a weak acid.
How does the dissociation of acetic acid differ from that of a strong acid?
The comparison between the dissociation of acetic acid (a weak acid) and a strong acid (hydrochloric acid, HCl) is shown below.
| Aspect | Acetic Acid (CH3COOH) | Hydrochloric Acid (HCl) |
| Degree of Dissociation | Partial dissociation 4 5 | Complete dissociation 6 |
| Dissociation Equation | CH3COOH ⇌ CH3COO- + H+ | HCl ⇌ H+ + Cl- |
| Concentration of H+ ions | Low | High |
| pH of Aqueous Solution | Slightly acidic (pH<7) 7 | Highly acidic (pH<<7) 8 |
| Conductivity in Water | Lower electrical conductivity | Higher electrical conductivity 9 |
| Reaction with Metals | Slow reaction (mild) | Rapid reaction (vigorous) |
| Strength of Acidic Effect | Weak | Strong |
In the dissociation of acetic acid, only a fraction of the molecules break apart into acetate ions (CH3COO-) and hydrogen ions (H+). This leads to a relatively low concentration of H+ ions, resulting in a weak acidic effect with a pH below 7 but closer to neutral.
On the other hand, hydrochloric acid fully dissociates into hydrogen ions (H+) and chloride ions (Cl-), resulting in a high concentration of H+ ions, leading to a strong acidic effect with a pH significantly below 7.
The higher concentration of H+ ions in the solution also makes strong acids better conductors of electricity compared to weak acids. 10 Additionally, strong acids react vigorously with metals, 11 whereas weak acids tend to show slower and milder reactions with metals.
Applications of acetic acid based on its weak acidic nature
Acetic acid’s weak acidic nature makes it suitable for various applications due to its ability to selectively donate protons to chemical reactions without being overly aggressive. Some of the notable applications include:
- Food Preservative and Flavoring Agent: Acetic acid, commonly known as vinegar when diluted in water, is used as a food preservative to inhibit the growth of bacteria and other microorganisms. 12 It also serves as a flavoring agent, adding a tangy taste to various culinary preparations.
- Household Cleaning Agent: Due to its mild acidity, acetic acid is an effective household cleaning agent. 13 It can be used to remove mineral deposits, stains, and rust from various surfaces like glass, tiles, and metal.
- pH Adjustment in Cosmetics and Personal Care Products: Acetic acid is used in the cosmetics and personal care industry to adjust the pH of products like shampoos, conditioners, and skin care formulations. It helps to stabilize and optimize the performance of these products.
- Textile Industry: Acetic acid is employed in the textile industry as a component of dyeing processes and for the production of synthetic fibers like acetate and triacetate. 14
- Chemical Synthesis: As a weak acid, acetic acid plays a vital role in various chemical synthesis reactions. It is used as a solvent and a catalyst in the production of pharmaceuticals, fragrances, and other organic compounds. 15
- Acid-Base Titrations: Acetic acid is a common weak acid used in educational settings during acid-base titration experiments to demonstrate the principles of neutralization reactions and pH determination.
In these applications, acetic acid’s weak acidic nature allows it to provide controlled acidity, minimizing the risk of damage or adverse effects while still performing essential functions in different industries and everyday products.
Further reading
Is H2CO3 (Carbonic Acid) a Strong or Weak Acid?
Is Formic Acid (HCOOH) a Strong or Weak Acid?
Is HCN a Strong or Weak Acid?
Is HBr a Strong or Weak Acid?
Is HI (Hydroiodic Acid) a Strong or Weak Acid?
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References
- 11.10: Weak Acids. (2016, May 9). Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/General_Chemistry/Book%3A_ChemPRIME_(Moore_et_al.)/11%3A_Reactions_in_Aqueous_Solutions/11.10%3A_Weak_Acids
- 5.1: Brønsted–Lowry Acids and Bases. (2015, April 1). Chemistry LibreTexts. https://chem.libretexts.org/Courses/University_of_Illinois_Springfield/UIS%3A_CHE_267_-_Organic_Chemistry_I_(Morsch)/Chapters/Chapter_02%3A_Acids_and_Bases/5.1%3A_Br%C3%B8nsted%E2%80%93Lowry_Acids_and_Bases
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- Ufl.edu https://christou.chem.ufl.edu/wp-content/uploads/sites/62/2017/01/Chapter-18-Acids-and-Bases-Week-1.pdf
- Fsu.edu https://chem.fsu.edu/chemlab/chm1046course/kaconstant.html
- Purdue.edu https://chemed.chem.purdue.edu/genchem/topicreview/bp/ch11/conjugat.php
- Elmhurst.edu http://chemistry.elmhurst.edu/vchembook/185strength.html
- Acid and Base Strength. (2013, October 2). Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Acids_and_Bases/Ionization_Constants/Acid_and_Base_Strength
- Metals reacting with acid (video) | Khan Academy. (n.d.). Khan Academy. https://www.khanacademy.org/science/in-in-class-10-chemistry-india/x87dd2847d57ee419:in-in-metals-and-non-metals/x87dd2847d57ee419:in-in-chemical-properties-of-metals/v/metals-reacting-with-acid-metals-and-non-metals-chemistry-khan-academy
- Marshall, D., Dickson, J., & Nguyen, N. (2016). Ensuring Food Safety in Insect Based Foods: Mitigating Microbiological and Other Foodborne Hazards. Insects as Sustainable Food Ingredients, 223–253. https://doi.org/10.1016/b978-0-12-802856-8.00008-9
- Selection and Use of Home Cleaning Products | New Mexico State University – BE BOLD. Shape the Future. (n.d.). Selection and Use of Home Cleaning Products | New Mexico State University – BE BOLD. Shape the Future. https://pubs.nmsu.edu/_g/G304/
- El Gabry, L. K. (n.d.). Replacement of Acetic Acid with Citric Acid in Dyeing of Textile Fabrics. (PDF) Replacement of Acetic Acid With Citric Acid in Dyeing of Textile Fabrics | L K El Gabry – Academia.edu. https://www.academia.edu/31029166/Replacement_of_Acetic_Acid_with_Citric_Acid_in_Dyeing_of_Textile_Fabrics
- Acetic acid. (n.d.). Acetic Acid. https://www.cs.mcgill.ca/~rwest/wikispeedia/wpcd/wp/a/Acetic_acid.htm
