A bottle of commercial vinegar contains 5% acetic acid, ch3cooh, by volume (95% water). the density of acetic acid is 1.05 g/ml and water is 1.00 g/ml. from this data calculate the concentration of acetic acid in vinegar in: molality, molarity, parts by mass, and the mole fraction.

See explanation.

Explanation:

Hello,

For this exercise, it is convenient to assume a basis of 5 g of acetic acid which is the solute and 95 g of water which is the solvent, in such a way, one proceeds as follows:

(a) Molarity:

Thus:

(b) Molality:

In this case, the moles were already computed and the mass of the solvent is in kilograms, thus:

(c) Parts by mass:

(d) Mole fraction:

In this case, the moles of water are required:

Since:

Best regards.

it is stable as it is in group 0 which have full outer shells of electrons