Conjugate acid The species formed when

Condensed states of matter liquids and solids. (16.1) Conduction bands the molecular orbitals that can be occupied by mobile electrons, which are free to travel throughout a metal crystal to conduct electricity or heat. (16.4) Conjugate acid the species formed when a proton is added to a base. (7.1)... 

Conjugate acid the species formed when a proton is added to a base. (14.1)... 

Conjugate acid The species formed when a base accepts a proton. 

Conjugate base The species formed when an acid donates a proton. 

Because HCN is the acid that forms when a proton is transferred to a cyanide ion, HCN is the conjugate acid of the base CN. In general, a conjugate acid of a base is the species formed when the base accepts a proton ... 

A conjugate acid is the molecule or ion formed when a proton is added to a base. A conjugate base is the species formed when a proton is removed from an acid. A pair of species differing by a single proton is called a conjugate acid-base pair. The word conjugate means joined together as a paiF. 

The products of proton transfer in aqueous solution may also react with water. For example, the CIST ion produced when HCN loses a proton to water can accept a proton from a water molecule and form HCN again. Therefore, according to the Bronsted definition, CN is a base it is called the conjugate base of the acid HCN. In general, a conjugate base of an acid is the species left when the acid donates a proton ... 

An important feature of the Brpnsted-Lowry concept is the idea that the product formed when an acid gives up a proton is a potential proton acceptor and is called the conjugate base of the parent acid. For example, when the species acidj gives up a proton, the species basej is formed, as shown by the reaction... 

The conjugate base of a Bronsted- Lowry add is the species that remains when a proton is removed from the acid. The conjugate acid of a Bronsted Lowry base is the species formed by adding a proton to the base. Together, an acid and its conjugate base (or a base and its conjugate add) are called a conjugate acid-base pair. 

When dealing with proton-transfer reactions, remember that the weaker a Bronsted-Lowry acid, the stronger its conjugate base. (Section 16.2) For example, H2, OH , NH3, and CH4 are exceedingly weak proton donors that have no tendency to act as acids in water. Thus, the species formed by removing one or more protons from them are extremely strong bases. All react readily with water, removing protons from H2O to form OH. Two representative reactions are ... 

The most important appHcation of metal alkoxides in reactions of the Friedel-Crafts type is that of aluminum phenoxide as a catalyst in phenol alkylation (205). Phenol is sufficientiy acidic to react with aluminum with the formation of (CgH O)2Al. Aluminum phenoxide, when dissolved in phenol, greatiy increases the acidic strength. It is beheved that, similar to alkoxoacids (206) an aluminum phenoxoacid is formed, which is a strong conjugate acid of the type HAl(OCgH )4. This acid is then the catalyticaHy active species (see Alkoxides, metal). 

As long as the buffer solution contains acetic acid as a major species, a small amount of hydroxide ion added to the solution will be neutralized completely. Figure 18-1 shows two hydroxide ions added to a portion of a buffer solution. When a hydroxide ion collides with a molecule of weak acid, proton transfer forms a water molecule and the conjugate base of the weak acid. As long as there are more weak acid molecules in the solution than the number of added hydroxide ions, the proton transfer reaction goes virtually to completion. Weak acid molecules change into conjugate base anions as they mop up added hydroxide. 

When a base accepts a proton, the species that is left is known as the conjugate acid. For every base, a conjugate acid is formed when the base gains a proton (see table for examples). 

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