an acid and a base that are the same except for an H+
-apex
The concept of conjugate acid-base pairs was proposed by G. N. Lewis in 1923. Later, this concept was further developed by G. S. Hammond in 1955, who introduced the idea of considering the relative stability of the conjugate acid-base pairs.
Conjugate pairs must be composed of weak acids and bases because strong acids and bases do not have the ability to donate or accept protons effectively. Weak acids and bases, on the other hand, can easily transfer protons between each other, making them suitable for forming conjugate pairs. This requirement ensures that the equilibrium between the acid and its conjugate base (or base and its conjugate acid) can be established and maintained.
2
Some examples of conjugate acid-base pairs are HCl and Cl-, H2O and OH-, NH3 and NH4+.
HI and I- H2O AND OH- HOCl and OCI-
Conjugate acid-base pairs have similar chemical properties because they differ by a proton. The conjugate acid is formed by gaining a proton, while the conjugate base is formed by losing a proton. This shared relationship ensures that they have similar reactivity and behavior in chemical reactions.
The concept of conjugate acid-base pairs was proposed by G. N. Lewis in 1923. Later, this concept was further developed by G. S. Hammond in 1955, who introduced the idea of considering the relative stability of the conjugate acid-base pairs.
Conjugate pairs must be composed of weak acids and bases because strong acids and bases do not have the ability to donate or accept protons effectively. Weak acids and bases, on the other hand, can easily transfer protons between each other, making them suitable for forming conjugate pairs. This requirement ensures that the equilibrium between the acid and its conjugate base (or base and its conjugate acid) can be established and maintained.
2
Some examples of conjugate acid-base pairs are HCl and Cl-, H2O and OH-, NH3 and NH4+.
HI and I- H2O AND OH- HOCl and OCI-
1-14
If acid is strong then its conjugate base must be weak, if conjugate base is strong it again accept the H+ ions so acid can neither be strong, similarly if base is strong its conjugate acid must be weak.
NH3 + H20 <----> NH4+ + OH- Ammonia is a weak base so it is the favored side of the equilbrium. Conjugate acid and base pairs only differ by a proton. So ammonia and ammonium are pairs and water and hydroxide ions are pairs. NH4+ + CN- <-------> HCN + NH3
In a chemical reaction, conjugate redox pairs are related because they involve the transfer of electrons between them. One species loses electrons (oxidized) while the other gains electrons (reduced). This exchange of electrons allows the reaction to proceed and maintain charge balance.
That's true. Complex and pure-imaginary solutions come in 'conjugate' pairs.
When ammonia (NH₃) is dissolved in water, it acts as a weak base and accepts a proton (H⁺) from water, forming ammonium (NH₄⁺) and hydroxide ions (OH⁻). The forward reaction is NH₃ + H₂O ⇌ NH₄⁺ + OH⁻. In the reverse reaction, ammonium can donate a proton back to hydroxide, reforming ammonia and water: NH₄⁺ + OH⁻ ⇌ NH₃ + H₂O. The conjugate acid-base pairs are (NH₃/NH₄⁺) and (H₂O/OH⁻).