Introduction:
When a weak acid (CH3COOH) and a strong base (NaOH) are mixed together, a neutralization reaction occurs. The reaction between CH3COOH and NaOH forms water and sodium acetate (CH3COONa). The molar conductivity of the mixture can be determined by considering the conductivities of the individual components and the degree of ionization.

Calculating the molar conductivity:
To calculate the molar conductivity of the mixture, we need to consider the conductivities of CH3COOH and NaOH and their respective degrees of ionization.

Conductivity of CH3COOH:
CH3COOH is a weak acid, so it partially dissociates in water. The degree of ionization is given by the formula:
Degree of ionization (α) = √(K / C)
Where K is the acid dissociation constant and C is the concentration of the acid.

For CH3COOH, the acid dissociation constant (Ka) is known. By substituting the values of Ka and C into the formula, we can determine the degree of ionization.

Conductivity of NaOH:
NaOH is a strong base, so it completely dissociates in water. Therefore, the degree of ionization for NaOH is 1.

Molar conductivity of the mixture:
The molar conductivity of the mixture is given by the formula:
Λmixture = ΛCH3COOH + ΛNaOH

Where ΛCH3COOH is the molar conductivity of CH3COOH and ΛNaOH is the molar conductivity of NaOH.

To calculate the molar conductivity of the mixture, we need to know the molar conductivities of CH3COOH and NaOH. These values can be obtained from experimental data or reference sources.

Conclusion:
In conclusion, to determine the molar conductivity of a mixture of 0.015M CH3COOH and 0.015M NaOH, we need to calculate the degree of ionization for CH3COOH and consider the molar conductivities of both components. By using the formula Λmixture = ΛCH3COOH + ΛNaOH, we can calculate the molar conductivity of the mixture.