Give 2 examples of miscible and immiscible liquids which dissolve in water
The Correct Answer and Explanation is:
Examples of Miscible Liquids:
- Ethanol and Water
Ethanol (C2H5OH) and water (H2O) are examples of miscible liquids. When mixed together, they form a homogeneous solution at any concentration. This is because both ethanol and water have similar intermolecular forces. Water molecules are polar, and ethanol contains both a hydrophilic (water-attracting) -OH group and a hydrophobic (water-repelling) hydrocarbon tail. The polarity of the -OH group allows the ethanol to interact favorably with water molecules, resulting in their complete dissolution. - Acetone and Water
Acetone (CH3COCH3) and water are also miscible. Acetone is a polar solvent and can form hydrogen bonds with water molecules, allowing it to dissolve completely in water. The interactions between acetone’s oxygen atom and water’s hydrogen atoms lead to the complete mixing of the two liquids in all proportions.
Examples of Immiscible Liquids:
- Oil and Water
Oil and water are classic examples of immiscible liquids. Water molecules are polar, while oil molecules are non-polar. The polar water molecules form strong hydrogen bonds with each other, making it difficult for them to interact with the non-polar oil molecules. As a result, oil and water separate into two distinct layers when combined, and they do not dissolve in one another. - Mercury and Water
Mercury (Hg) and water are immiscible due to their different intermolecular forces. Mercury is a metal that forms metallic bonds, and water is polar. The cohesive forces between mercury atoms are much stronger than any interaction between mercury and water molecules, leading to the separation of the two liquids. This immiscibility is a result of the mercury’s high surface tension and the fact that its atoms do not readily form bonds with water molecules.
Explanation:
The key difference between miscible and immiscible liquids lies in their molecular interactions. Miscible liquids, such as ethanol in water, dissolve because their molecular structures allow for favorable interactions between them, such as hydrogen bonding or dipole-dipole interactions. On the other hand, immiscible liquids, like oil and water, fail to mix because their molecular structures result in incompatible interactions—polar water molecules cannot interact well with non-polar oil molecules, preventing dissolution.
