How to Calculate pH at Equivalence Point in Titration?

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To calculate the pH at the equivalence point of the titration between 0.2500 M CH3COONa and 0.1300 M HCl, it is essential to recognize that at this point, all acetate ions (CH3COO−) have reacted with hydrogen ions (H+) to form acetic acid (CH3COOH). The volume of HCl required to reach the equivalence point is determined to be 19.23 mL. Since acetic acid is a weak acid, the pH at the equivalence point will be greater than 7. The dissociation constant for acetic acid (Ka = 1.8 x 10^-5) is crucial for calculating the pH, as it will allow for the determination of the concentration of hydrogen ions in the resulting solution. The calculations involve using the equilibrium expression for the dissociation of acetic acid to find the pH accurately.
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A 10.00 mL solution of 0.2500 M CH3COONa is titrated with 0.1300 M HCl to the equivalence point.
CH3COO− + H+ → CH3COOH
volume of HCl required=19.23 mL

Calculate the pH of the solution at the equivalence point.

I've tried this a million ways and still keep getting it wrong. Also, my chemistry prof doesn't respond or have office hours so I'm kind of on my own :( Thank you in advance for your help :).
 
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You need the dissociation constant for acetic acid. It is a weak acid, and therefore the equivalence point pH will be greater than 7.
 
Dissociation constant for CH3COOH
Ka = 1.8 x 10^-5
 

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