The pH at the equivalence point when a solution of 0.01 M-CH3 COOH is titrated with a solution o

step 1 Hello students for this question my reaction would be CH3 CW Racting with N -A -O -H and it will

The pH at the equivalence point when a solution of 0.01...

The $\mathrm{pH}$ at the equivalence point when a solution of $0.01 \mathrm{M}-\mathrm{CH}_{3} \mathrm{COOH}$ is titrated with a solution of $0.01 \mathrm{M}-\mathrm{NaOH}$, is $\left(\mathrm{p} K_{\mathrm{a}}\right.$ of $\mathrm{CH}_{3} \mathrm{COOH}=4.7, \log 5=0.7$ ) (a) $10.5$ (b) $3.5$ (c) $10.35$ (d) $3.65$

The $\mathrm{pH}$ at the equivalence point when a solution of $0.01 \mathrm{M}-\mathrm{CH}_{3} \mathrm{COOH}$ is titrated with a solution of $0.01 \mathrm{M}-\mathrm{NaOH}$, is $\left(\mathrm{p} K_{\mathrm{a}}\right.$
of $\mathrm{CH}_{3} \mathrm{COOH}=4.7, \log 5=0.7$ )
(a) $10.5$
(b) $3.5$
(c) $10.35$
(d) $3.65$

Key Concepts

Titration of a Weak Acid with a Strong Base

This concept involves the gradual addition of a strong base to a weak acid, wherein at the equivalence point all of the weak acid has been converted into its corresponding conjugate base. The titration process highlights the chemical transformation and the shift in acid?base properties, leading to a solution that is basic in nature due to the hydrolysis of the conjugate base.

Equivalence Point

The equivalence point in a titration is the stage at which the quantity of titrant added equals the amount of the substance being titrated, as determined by stoichiometry. In the weak acid–strong base titration, this means that all the initially present weak acid has been neutralized to form its conjugate base, which subsequently undergoes hydrolysis affecting the final pH.

Conjugate Base Hydrolysis

At the equivalence point in a weak acid–strong base titration, the conjugate base that forms can react with water, a process known as hydrolysis. This reaction generates hydroxide ions, thereby increasing the pH of the solution above neutral. The extent of this hydrolysis depends on the strength of the conjugate base, which is inversely related to the acid's strength.

Relationship between Ka and Kb

Ka (acid dissociation constant) and Kb (base dissociation constant) are related by the ion?product constant for water (Kw). For a weak acid and its conjugate base, knowing the Ka allows calculation of the Kb for the conjugate base using the formula Kb = Kw/Ka. This relationship is fundamental in computing the pH at the equivalence point in a weak acid–strong base titration.

pH Calculation in Titration Curves

Calculating the pH at the equivalence point of a titration involving a weak acid and a strong base involves accounting for the hydrolysis of the conjugate base. The determination of pH requires solving the equilibrium for the weak base, often using approximations based on the square root of the product of the base’s dissociation constant and its concentration, followed by the conversion of hydroxide ion concentration to pOH and then to pH.

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