Answer :
Titration is a process used to determine the concentration of an unknown solution by reacting it with a solution of a known concentration. pH at the equivalence point when titrating 5.00 ml of 0.10 M acetic acid with 5.00 ml of 0.10 M KOH is 4.76.
Acetic acid is a weak acid, which means it does not dissociate completely in water. Its dissociation can be represented by the following equation: [tex]CH_{3} COOH + H_{2}O = CH_{3} COO- + H_{3}O[/tex]
The Ka value for acetic acid Given, which is a measure of its acidity. In the presence of a strong base like KOH, the base reacts with the acid to form water and a salt: [tex]CH_{3} COOH + H_{2}O = CH_{3} COO- + H_{3}O[/tex]
At the equivalence point, the number of moles of acid equals the number of moles of base added. This means that all the acetic acid has been neutralized, and the solution contains only the acetate ion and hydroxide ion from the KOH. The pH of the solution at the equivalence point is determined by the hydrolysis of the acetate ion.
[tex]CH_{3} COOH + H_{2}O = CH_{3} COO- + OH[/tex]
The equilibrium constant for this reaction is Kw/Ka, where Kw is the ionization constant of water. At 25°C, Kw/Ka is equal to [tex]5.6 . 10^{-10}[/tex]. Therefore, the pH at the equivalence point can be calculated using the following equation: pH = pKa + log([base]/[acid])
At the equivalence point, [base] = [acid], so the equation simplifies to: pH = pKa + log(1), pH = pKa, Substituting the value of pKa for acetic acid (4.76) into the equation gives: pH = 4.76
Therefore, the pH at the equivalence point when titrating 5.00 ml of 0.10 M acetic acid with 5.00 ml of 0.10 M KOH is 4.76.
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