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,
A 0.10 M solution of acetic acid (CH3COOH, Ka = 1.8 x 10^-5) is titrated with a 0.0250 M solution of magnesium hydroxide (Mg(OH)2). If 10.0 mL of the acid solution is titrated with 10.0 mL of the base solution, what is the pH of the resulting solution?
Firefly luciferin exhibits three rings. Identify which of the rings are aromatic. Identify which lone pairs are involved in establishing aromaticity. The lone pairs are labeled A-D below.
A 0.10 M solution of acetic acid (CH3COOH, Ka = 1.8 x 10^-5) is titrated with a 0.0250 M solution of magnesium hydroxide (Mg(OH)2). If 10.0 mL of the acid solution is titrated with 10.0 mL of the base solution, what is the pH of the resulting solution?
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