Ions in aqueous solution that are surrounded by polar water molecules are said to be saturated.
is it true or false?
false.
This statement is false. When ions are surrounded by polar water molecules, they are referred to as hydrated ions, not saturated.
To understand why, let's break down the statement and explain the concepts involved:
1. Ions in aqueous solution: Aqueous solution refers to a solution where water is the solvent, and ions are present in the solution. When certain substances dissolve in water, they dissociate into ions, creating an ionic solution.
2. Surrounded by polar water molecules: Water is a polar molecule, meaning it has a partial positive charge on its hydrogen atoms and a partial negative charge on its oxygen atom. This polarity allows water molecules to form electrostatic interactions with ions, attracting and surrounding them.
3. Saturated: Saturated refers to a condition when a solvent, usually a liquid, has dissolved as much solute (the substance being dissolved) as it can at a given temperature and pressure. When a solution is saturated, it cannot dissolve any more of the solute.
Therefore, the statement's claim that ions in aqueous solution surrounded by polar water molecules are saturated is incorrect. Being surrounded by water molecules doesn't necessarily mean the solution is saturated. The solubility of an ionic compound in water determines whether the solution is saturated, unsaturated, or supersaturated.
False.
Ions in aqueous solution that are surrounded by polar water molecules are not said to be saturated. The term "saturated" is commonly used to describe the maximum amount of solute that can dissolve in a solvent at a specific temperature. In the context of ions in aqueous solution, the term "solvated" is more appropriate. When ions dissolve in water, they become surrounded by water molecules, forming a solvation shell. This solvation process occurs through electrostatic interactions between the water molecules and the charged ions.