Solubility and the Dissolving Process Chapter 7.2 and 7.3

What is solubility? The amount of solute that will dissolve into a solvent (at a certain pressure and temperature) Remember, solute is the smaller amount of a substance and the solvent is the larger portion of what is combined

Different substances have different solubilities… Solubilities of some ionic compounds in water

How to describe how much solute is dissolved in the solvent… Concentration—the amount of a particular substance in a solution – Large amount of solute = concentrated solution – Small amount of solute = dilute solution

How concentrated are solution? Saturated solution—a solution that cannot dissolve anymore solute into it (It’s full!) Unsaturated solution—a solution where more solute can still be dissolved into it (“contains less solute than the saturated solution”)

Temperature… The solubility increases as the temperature of the solution increases (if you heat up the solution, more can be dissolved into it!) Supersaturated solution—a solution that holds more dissolve solute than the regular equilibrium saturated state

How to make a crystal… Heat up a solution, dissolve more solute in than can normally dissolve, then cool back down the solution Add one extra bit of solute (a crystal of solute”) and the whole solution and extra solute will crystallize out!

What affects the dissolving process? Stirring or shaking (helps solute dissolve faster by bumping them against the solute particles faster) Heating up the solvent (particles move faster with more energy) Larger surface area  increases dissolving rate (more area of the solute to interact with the solvent)

Solute affect the physical properties of solutions… Adding solute will cause… – The boiling point of a solution to increase (boiling point elevation) – The freezing point of a solution to decrease (freezing point depression) So, instead of water freezing at 0 degrees Celsius, it freezes at -15 degrees Celsius.

Your mission… …if you choose to accept it….