A solution is prepared by dissolving 12.5 g of KBr in 20 mL of water at 60^∘ C (see Figure 9.3

step 1 Hi students. So in this question we need to tell when we go the solution to 10 degrees Celsius t

A solution is prepared by dissolving 12.5 g of KBr in 20...

A solution is prepared by dissolving $12.5 \mathrm{~g}$ of $\mathrm{KBr}$ in $20 \mathrm{~mL}$ of water at $60^{\circ} \mathrm{C}$ (see Figure 9.3 ). Is this solution saturated, unsaturated, or supersaturated? What will happen if the solution is cooled to $10^{\circ} \mathrm{C}$ ?

Key Concepts

Saturated, Unsaturated, and Supersaturated Solutions

A saturated solution is one in which the solvent contains the maximum amount of dissolved solute possible at a given temperature, with any excess solute remaining undissolved. An unsaturated solution contains less solute than the maximum possible, meaning additional solute could still be dissolved. A supersaturated solution has dissolved more solute than would normally be possible at a particular temperature; it is metastable and any small disturbance can prompt rapid precipitation of the excess solute.

Temperature Dependence of Solubility

The solubility of most solids in water is dependent on temperature, often increasing with an increase in temperature and decreasing with a reduction in temperature. This relationship is usually depicted by a solubility curve, which indicates how much solute can be dissolved at different temperatures. Changes in temperature can therefore alter the state of a solution, potentially causing an unsaturated solution at high temperatures to become saturated or even supersaturated when cooled.

Solubility

Solubility describes the maximum quantity of a solute that can dissolve in a given quantity of solvent at a specific temperature, forming a homogeneous solution. It is typically expressed in units such as grams of solute per 100 grams of solvent. This concept is central to understanding whether a solution is saturated, unsaturated, or supersaturated, as it dictates the limit of solute that can be accommodated under equilibrium conditions.

Precipitation

Precipitation is the process by which a solute comes out of solution in solid form when the solution becomes saturated due to changes in conditions, such as a decrease in temperature. When a solution that initially holds more solute in a dissolved state (because of higher temperature) is cooled, its solubility decreases, and the excess solute crystallizes or precipitates out to reestablish equilibrium.

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