buffer equation - vertaling naar arabisch
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buffer equation - vertaling naar arabisch

EQUATION USED TO ESTIMATE THE PH OF A WEAK ACID OR BASE SOLUTION
Henderson-Hasselbach equation; Henderson-Hasselbach Equation; Henderson-Hasselhoff equation; Hasselhoff equation; Henderson-Hasselhoff; Henderson hasselbach; Henderson-Hasselbalch; Henderson-Hasselbach; Henderson-Hasselbalch Equation; Henderson Hasselbach; Henderson Hasselbalch; Henderson Hasselbalch equation; Henderson hasselboch; Henderson-Hasselbalch equation; H-H; Henderson–Hasselbach equation; Henderson equation; Buffer equation; Henderson Hasselbach equation; Kristipati-Arivoli Equation
  • 1=p''K''<sub>a</sub> = 4.7}}) with alkali

buffer equation         
‎ مُعادَلَةُ الدَّارِئ‎
Henderson Hasselbalch equation         
‎ مَعادَلَةُ هندرسن-هاسلبالخ‎
Henderson-Hasselbalch equation         
مَعادَلَةُ هندرسن-هاسلبالخ

Definitie

buffer state
(buffer states)
A buffer state is a peaceful country situated between two or more larger hostile countries.
Turkey and Greece were buffer states against the former Soviet Union.
N-COUNT

Wikipedia

Henderson–Hasselbalch equation

In chemistry and biochemistry, the Henderson–Hasselbalch equation

relates the pH of a chemical solution of a weak acid to the numerical value of the acid dissociation constant, Ka, of acid and the ratio of the concentrations, [ Base ] [ Acid ] {\displaystyle {\frac {[{\ce {Base}}]}{[{\ce {Acid}}]}}} of the acid and its conjugate base in an equilibrium.
H A ( a c i d ) A ( b a s e ) + H + {\displaystyle \mathrm {{\underset {(acid)}{HA}}\leftrightharpoons {\underset {(base)}{A^{-}}}+H^{+}} }

For example, the acid may be acetic acid

C H 3 C O 2 H C H 3 C O 2 + H + {\displaystyle \mathrm {CH_{3}CO_{2}H\leftrightharpoons CH_{3}CO_{2}^{-}+H^{+}} }

The Henderson–Hasselbalch equation can be used to estimate the pH of a buffer solution by approximating the actual concentration ratio as the ratio of the analytical concentrations of the acid and of a salt, MA.

The equation can also be applied to bases by specifying the protonated form of the base as the acid. For example, with an amine, R N H 2 {\displaystyle \mathrm {RNH_{2}} }

R N H 3 + R N H 2 + H + {\displaystyle \mathrm {RNH_{3}^{+}\leftrightharpoons RNH_{2}+H^{+}} }