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A conjugate acid, within the Brønsted–Lowry acid–base theory, is a chemical compound formed when an acid gives a proton ... lactic acid, CH 3 CH(OH)CO ...
The following reaction represents the general reaction between a base (B) and water to produce a conjugate acid (BH +) and a conjugate base (OH −): [3] + + + The equilibrium constant, K b, for this reaction can be found using the following general equation: [3]
The acid, HA, is a proton donor which can lose a proton to become its conjugate base, A −. The base, B, is a proton acceptor which can become its conjugate acid, HB + . Most acid–base reactions are fast, so the substances in the reaction are usually in dynamic equilibrium with each other.
This is done because the H + concentration is not a part of the reaction, whereas the OH − concentration is. The pOH is defined as: = [] If we multiply the equilibrium constants of a conjugate acid (such as NH 4 +) and a conjugate base (such as NH 3) we obtain:
Here, one molecule of water acts as an acid, donating an H + and forming the conjugate base, OH −, and a second molecule of water acts as a base, accepting the H + ion and forming the conjugate acid, H 3 O +. As an example of water acting as an acid, consider an aqueous solution of pyridine, C 5 H 5 N.
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A Lewis base is often a Brønsted–Lowry base as it can donate a pair of electrons to H +; [11] the proton is a Lewis acid as it can accept a pair of electrons. The conjugate base of a Brønsted–Lowry acid is also a Lewis base as loss of H + from the acid leaves those electrons which were used for the A—H bond as a lone pair on the ...
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