8. Which of these common laboratory solvents are polar? Circle all that apply: b) cyclohexane (C6H12) a) Water (H20) c) ethanol (CH3CH20H) d) acetic acid (CH3C0OH) e) neo-pentane (C$H12)

a) Water (H20)

c) ethanol (CH3CH20H)

d) acetic acid

Explanation:

In chemistry, the parameter that measures its polarity and confers solubilization properties of different solutes is called the polarity of a solvent. In general, chemical reactions take place in a homogeneous phase, since, for two species to come into contact, they must be in the same phase. In solution, the reactive species enjoy greater freedom of movement and diffuse in the total volume of the solvent, thus increasing the probability of collision between them.

The solvent must act on the solute by solvating it and overcoming the intermolecular forces that hold it together, but without giving rise to the reaction. Depending on the nature of the solute and the solvent, the solvation forces between the two can be of different types: hydrogen bridges, polar interactions and London forces.

The suitable solvent usually has chemical and structural characteristics similar to those of the compound to be dissolved. The polarity and, consequently, the solubility of the organic compounds in polar solvents, increases with the decrease in the length of the hydrocarbon chain, the presence of polar functional groups and the ability to form hydrogen bonds with the solvent.

The 3 chemical substances indicated as polar solvents are found within the group of protic polar solvents.

Polar solvents: These are substances in whose molecules the distribution of the electronic cloud is asymmetric; therefore, the molecule has a positive and a negative pole separated by a certain distance. There is a permanent dipole. The classic example of polar solvent is water. Low molecular mass alcohols also belong to this type