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When a liquid is placed in a container, such as a buret, a meniscus forms at the surface. This meniscus may be concave or convex, influenced by the balance between cohesive and adhesive forces. A meniscus is essentially the curve that you see at the surface of a liquid. It's created because of the interaction between the liquid molecules and the molecules of the container walls. When the adhesive forces—those between the liquid and the container—are stronger than the cohesive forces within the liquid, the liquid will climb up the sides of the container slightly. This leads to a concave meniscus, like the one seen with water. On the other hand, if cohesive forces are stronger, a convex meniscus will form, which is often seen with mercury.

Cohesive forces are the attractive forces between like molecules within a liquid. These forces are responsible for holding the liquid together. In simple terms, they help liquid molecules "stick" to each other. These cohesive forces are key players in determining the shape and behavior of the liquid's surface.
When cohesive forces are strong, they can pull the surface molecules towards the bulk of the liquid, creating tension. This strong internal attraction among the molecules is what contributes to the formation of a convex meniscus in some liquids like mercury. In such cases, the cohesive forces overpower the adhesive forces, causing the liquid surface to bend downward at the sides, giving the characteristic bulging appearance.

Adhesive forces refer to the attractive forces between unlike molecules, such as those between a liquid and the surface of a container. These forces explain why some liquids tend to "stick" to the sides of the container. Adhesive forces play a significant role in how a liquid behaves at its boundary.
For example, in a buret or a glass tube, if the adhesive forces between the liquid molecules and the glass are strong, the liquid will spread more on the surface and create a concave meniscus. This effect is even more pronounced when the adhesive forces outweigh the cohesive forces pulling the liquid particles inward. Hence, water in a glass or plastic container typically shows a concave meniscus due to the strong adhesive forces between water and container materials.

Intermolecular forces are the forces of attraction that occur between molecules in a liquid. These forces are crucial in giving a liquid its unique set of properties. Intermolecular forces include a range of interactions, such as van der Waals forces, hydrogen bonding, and dipole-dipole interactions.
Strong intermolecular forces result in higher surface tension, which leads to significant meniscus formation. The balance or imbalance between these intermolecular forces influences the liquid's overall behavior and interactions with surfaces. Surface tension, an effect of these forces, acts like an invisible film on the liquid surface, resisting external influence and giving rise to phenomena like meniscus formation and capillary action.

The properties of a liquid, such as viscosity, density, and especially surface tension, heavily influence how it behaves in various conditions. Surface tension is particularly important as it dictates how the liquid interacts with surfaces, including the formation of a meniscus. Liquids with high surface tension, like mercury, tend to form convex menisci because their strong cohesive forces prevent them from wetting surfaces easily.
Understanding a liquid's properties involves looking at how its molecules interact with each other and with different surfaces. These molecular interactions, driven by intermolecular forces, can explain why some liquids easily climb surfaces while others do not. Thus, by studying liquid properties, we get insights into the broader behaviors, including how they spread, shape, and interact in containers.