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The self-ionization of water (also autoionization of water, autoprotolysis of water, autodissociation of water, or simply dissociation of water) is an ionization reaction in pure water or in an aqueous solution, in which a water molecule, H 2 O, deprotonates (loses the nucleus of one of its hydrogen atoms) to become a hydroxide ion, OH −.
Buffer solutions resist pH change because of a chemical equilibrium between the weak acid HA and its conjugate base A −: HA ⇌ H + + A − When some strong acid is added to an equilibrium mixture of the weak acid and its conjugate base, hydrogen ions (H + ) are added, and the equilibrium is shifted to the left, in accordance with Le ...
Because the relationship pK b = pK w − pK a holds only in aqueous solutions (though analogous relationships apply for other amphoteric solvents), subdisciplines of chemistry like organic chemistry that usually deal with nonaqueous solutions generally do not use pK b as a measure of basicity.
A conjugate acid, within the Brønsted–Lowry acid–base theory, is a chemical compound formed when an acid gives a proton (H +) to a base—in other words, it is a base with a hydrogen ion added to it, as it loses a hydrogen ion in the reverse reaction.
If positive and negative charges are both present in equal amounts, then this is the isoelectric point. Thus, the PZC refers to the absence of any type of surface charge, while the IEP refers to a state of neutral net surface charge. The difference between the two, therefore, is the quantity of charged sites at the point of net zero charge.
In biochemistry and in biological fluids, at pH = 7, it is thus important to note that the reduction potential of the protons ( H +) into hydrogen gas H 2 is no longer zero as with the standard hydrogen electrode (SHE) at 1 M H + (pH = 0) in classical electrochemistry, but that E red = − 0.414 V {\displaystyle E_{\text{red}}=-0.414\mathrm {V ...
In chemistry, biochemistry, and pharmacology, a dissociation constant (K D) is a specific type of equilibrium constant that measures the propensity of a larger object to separate (dissociate) reversibly into smaller components, as when a complex falls apart into its component molecules, or when a salt splits up into its component ions.
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