By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution:(c) K₂Cr₂O₇

Verified step by step guidance

1. Identify the solubility of K_2Cr_2O_7 in water at 40 °C from Figure 13.15. This will tell you how many grams of K_2Cr_2O_7 can dissolve in 100 g of water at this temperature.
2. Compare the given amount of K_2Cr_2O_7 (40.0 g) to the solubility value obtained from the figure.
3. If the solubility value is greater than or equal to 40.0 g, the solution will be unsaturated or just saturated, meaning all the K_2Cr_2O_7 can dissolve.
4. If the solubility value is less than 40.0 g, the solution will be saturated, and some of the K_2Cr_2O_7 will remain undissolved.
5. Conclude whether the addition of 40.0 g of K_2Cr_2O_7 to 100 g of water at 40 °C results in a saturated solution based on the comparison.

Key Concepts

Solubility

Solubility is the maximum amount of a solute that can dissolve in a given quantity of solvent at a specific temperature. It is typically expressed in grams of solute per 100 grams of solvent. Understanding solubility is crucial for determining whether a solution can become saturated, meaning no more solute can dissolve in the solvent at that temperature.

Saturated Solution

A saturated solution is one in which the maximum amount of solute has been dissolved in the solvent at a given temperature, resulting in an equilibrium between dissolved and undissolved solute. When additional solute is added to a saturated solution, it will not dissolve, indicating that the solubility limit has been reached.

Ionic Compounds and Their Solubility

Ionic compounds, such as K₂Cr₂O₇, dissociate into their constituent ions when dissolved in water. The solubility of these compounds varies widely depending on the specific ions involved and the temperature. Knowledge of the solubility rules helps predict whether a particular ionic solid will dissolve in water and to what extent.