use the bronsted-lowry model to label the acid-base pairs in the following equation for the ionization of water: H20(L) + H20(L) <--> H30+(AQ) + OH-(AQ). EXAPLAIN
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The Brønsted-Lowry model is a theory of acids and bases based on their ability to donate or accept protons (H+ ions). According to this model, an acid is a species that donates a proton, while a base is a species that accepts a proton.
In the equation for the ionization of water, we have H2O(L) + H2O(L) ⇌ H3O+(aq) + OH-(aq). Let's analyze the acid-base pairs involved:
1. Acid: In this equation, one of the water molecules transfers a proton to the other water molecule. The water molecule that donates the proton (H+) is acting as an acid. Therefore, it is labeled as the acid. So, H2O(L) is the acid in this equation.
2. Base: The other water molecule accepts the proton (H+). It acts as a base by accepting this proton. Therefore, it is labeled as the base. So, H2O(L) is the base in this equation.
3. Conjugate acid: After one water molecule has donated its proton to the other water molecule, it becomes positively charged and is now referred to as the hydronium ion (H3O+). The species formed when the base accepts a proton is labeled as the conjugate acid. So, H3O+(aq) is the conjugate acid in this equation.
4. Conjugate base: The other water molecule, after accepting the proton, loses its positive charge to form the hydroxide ion (OH-). The species formed when the acid donates the proton is labeled as the conjugate base. So, OH-(aq) is the conjugate base in this equation.
To summarize:
- H2O(L) is the acid.
- H2O(L) is the base.
- H3O+(aq) is the conjugate acid.
- OH-(aq) is the conjugate base.
The Brønsted-Lowry model helps us understand the transfer of protons in acid-base reactions and provides a framework for identifying the acid-base pairs involved.