To calculate the pH at the equivalence point, we first need to determine the stoichiometry of the reaction between acetic acid and sodium hydroxide.

The balanced equation for the reaction between acetic acid and sodium hydroxide is:

CH3COOH + NaOH → CH3COONa + H2O

From the balanced equation, we can see that one mole of acetic acid reacts with one mole of sodium hydroxide to produce one mole of sodium acetate and one mole of water. This means that at the equivalence point, the moles of acetic acid will be equal to the moles of sodium hydroxide.

Since we have a 0.10 M acetic acid solution, we can calculate the initial moles of acetic acid using the formula:

Moles = Concentration x Volume

The volume of the acetic acid solution is unknown, so we will use "V" to represent it.

Moles of acetic acid = 0.10 M x V

At the equivalence point, the moles of acetic acid will be equal to the moles of sodium hydroxide. Therefore, the moles of sodium hydroxide can be calculated using the following formula:

Moles of sodium hydroxide = 0.15 M x V

Since the moles of acetic acid and sodium hydroxide are equal at the equivalence point, we can set up the following equation:

0.10 M x V = 0.15 M x V

By canceling out the common factor of "V", we can simplify the equation to:

0.10 M = 0.15 M

Since the concentrations are not equal, this equation cannot be true. Therefore, there is no equivalence point in this titration.

As a result, we cannot directly calculate the pH at the equivalence point of this titration.

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