The K a of the amino acid serine if it is 86.3 % dissociated at pH of 9.95 has to be determined. Concept Introduction: Henderson-Hasselbalch equation is an equation which describes the derivation of pH as a measure of acidity in biological and chemical systems. This equation can be used to find the equilibrium pH in acid-base reaction and also for estimating the pH of a buffer solution. pH = pK a + log [ Conjugate base ] [ Weak acid ] p K a is analogues to pH and it is indicating the tendency of the compound to give up its proton. Lower p K a value stands for stronger acid. A weak acid (it is partially dissociated in aqueous solution) equilibrium can be represented as follows, H A W e a k a c i d ⇄ H + + A C o n j u g a t e b a s e −
The K a of the amino acid serine if it is 86.3 % dissociated at pH of 9.95 has to be determined. Concept Introduction: Henderson-Hasselbalch equation is an equation which describes the derivation of pH as a measure of acidity in biological and chemical systems. This equation can be used to find the equilibrium pH in acid-base reaction and also for estimating the pH of a buffer solution. pH = pK a + log [ Conjugate base ] [ Weak acid ] p K a is analogues to pH and it is indicating the tendency of the compound to give up its proton. Lower p K a value stands for stronger acid. A weak acid (it is partially dissociated in aqueous solution) equilibrium can be represented as follows, H A W e a k a c i d ⇄ H + + A C o n j u g a t e b a s e −
Solution Summary: The author explains the Henderson-Hasselbalch equation, which describes the derivation of pH as a measure of acidity in biological and chemical systems.
The Ka of the amino acid serine if it is 86.3% dissociated at pH of 9.95 has to be determined.
Concept Introduction:
Henderson-Hasselbalch equation is an equation which describes the derivation of pH as a measure of acidity in biological and chemical systems. This equation can be used to find the equilibrium pH in acid-base reaction and also for estimating the pH of a buffer solution.
pH=pKa+log[Conjugatebase][Weakacid]
pKa is analogues to pH and it is indicating the tendency of the compound to give up its proton. Lower pKa value stands for stronger acid.
A weak acid (it is partially dissociated in aqueous solution) equilibrium can be represented as follows,
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