10 mL of M/5 CH3COONa solution is titrated with M/5 HCl solution. The ...
Introduction:
In this titration, a M/5 CH3COONa solution (sodium acetate) is being titrated with a M/5 HCl solution (hydrochloric acid). The pH value at the equivalence point can be determined by considering the acid-base properties of the solutions involved and the reaction that occurs during the titration.
Equation:
The reaction between sodium acetate and hydrochloric acid can be represented by the following equation:
CH3COONa + HCl → CH3COOH + NaCl
Equivalence Point:
The equivalence point in a titration occurs when the number of moles of acid is equal to the number of moles of base or vice versa. In this case, at the equivalence point, all the sodium acetate will react with hydrochloric acid to form acetic acid and sodium chloride.
pH at Equivalence Point:
The pH at the equivalence point can be determined by considering the nature of the products formed during the reaction. Acetic acid (CH3COOH) is a weak acid and sodium chloride (NaCl) is a neutral salt.
Acetic Acid:
Acetic acid is a weak acid, meaning that it does not completely dissociate in water. It undergoes a partial ionization:
CH3COOH ⇌ CH3COO- + H+
At the equivalence point, all the sodium acetate has reacted with hydrochloric acid, resulting in the formation of acetic acid. Since acetic acid is a weak acid, the concentration of H+ ions will be relatively low.
pH Calculation:
To calculate the pH at the equivalence point, we need to consider the dissociation of water. Water undergoes self-ionization:
H2O ⇌ H+ + OH-
The concentration of H+ ions in pure water (at 25°C) is 1 x 10^-7 M. However, in the presence of acetic acid, the concentration of H+ ions will be slightly higher. Therefore, the pH at the equivalence point will be slightly acidic, but it will not be as low as the pH of a strong acid.
Conclusion:
The pH at the equivalence point of the titration between M/5 CH3COONa and M/5 HCl will be slightly acidic, but it will not be as low as the pH of a strong acid. This is because acetic acid, which is a weak acid, is formed during the reaction. The exact pH value will depend on the concentrations of the solutions and the dissociation constant of acetic acid (pKa value).