IB Chemistry Topic R3.1.3 Amphiprotic Species Revision Notes (SL/HL)

IB Chemistry Topic R3.1.3 Amphiprotic Species Revision Notes (SL/HL) | RevisionDojo

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Amphiprotic Species: Acting as Both Acids and Bases

Definition

Amphiprotic species

An amphiprotic species is a chemical species that can either donate a proton (acting as an acid) or accept a proton (acting as a base), depending on the reaction conditions.

This dual behavior enables amphiprotic species to play critical roles in chemical and biological systems.

Example

Common examples of amphiprotic species:

Water (H₂O)
Hydrogencarbonate ion (HCO₃⁻)
Hydrogen sulfate ion (HSO₄⁻)

Hint

Amphiprotic species are always involved in proton transfer reactions.
Look for a species that has a transferable hydrogen and can both donate and accept a proton to identify amphiprotic behavior!

Water: The Quintessential Amphiprotic Species

Water (H₂O) is the most well-known amphiprotic species.
It can act as both an acid and a base, depending on its reaction partner.

Water Acting as an Acid

When water reacts with a base, it donates a proton (H⁺), acting as an acid.
For example, in its reaction with ammonia (NH₃):$$
\text{H₂O} + \text{NH₃} \rightarrow \text{NH₄⁺} + \text{OH⁻}
$$
Here, water donates a proton to ammonia, forming the ammonium ion (NH₄⁺) and hydroxide ion (OH⁻).

Water Acting as a Base

When water reacts with an acid, it accepts a proton (H⁺), acting as a base.

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Amphiprotic Species: Acting as Both Acids and Bases

Definition

Amphiprotic species

An amphiprotic species is a chemical species that can either donate a proton (acting as an acid) or accept a proton (acting as a base), depending on the reaction conditions.

This dual behavior enables amphiprotic species to play critical roles in chemical and biological systems.

Example

Common examples of amphiprotic species:

Water (H₂O)
Hydrogencarbonate ion (HCO₃⁻)
Hydrogen sulfate ion (HSO₄⁻)

Hint

Amphiprotic species are always involved in proton transfer reactions.
Look for a species that has a transferable hydrogen and can both donate and accept a proton to identify amphiprotic behavior!

Water: The Quintessential Amphiprotic Species

Water (H₂O) is the most well-known amphiprotic species.
It can act as both an acid and a base, depending on its reaction partner.

Water Acting as an Acid

When water reacts with a base, it donates a proton (H⁺), acting as an acid.
For example, in its reaction with ammonia (NH₃):$$
\text{H₂O} + \text{NH₃} \rightarrow \text{NH₄⁺} + \text{OH⁻}
$$
Here, water donates a proton to ammonia, forming the ammonium ion (NH₄⁺) and hydroxide ion (OH⁻).

Water Acting as a Base

When water reacts with an acid, it accepts a proton (H⁺), acting as a base.

Definition

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Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

IB Chemistry R3.1.3 Amphiprotic Species Notes

Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

Amphiprotic Species: Acting as Both Acids and Bases

Water: The Quintessential Amphiprotic Species

Water Acting as an Acid

Water Acting as a Base

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Amphiprotic Species: Acting as Both Acids and Bases

Water: The Quintessential Amphiprotic Species

Water Acting as an Acid

Water Acting as a Base

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Duis aute irure dolor in reprehenderit

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