1. Solubility

2. Soluble the solutes ability to dissolve in a solvent
Solubility is the property of a substance (solute) to dissolve in another substance (solvent); solutions are characterized by their capacity to do so
Soluble the solutes ability to dissolve in a solvent
Insoluble the solute is not able to dissolve in a solvent
aqueous solutions of KMnO4
CdS
PbS
Ni(OH)2
Al(OH)3

3. Solubility is the property of a substance (solute) to dissolve in another substance (solvent).
Measured in terms of the maximum amount of solute dissolved in a solvent at a specific temperature
The resulting solution is called a saturated solution
Certain substances are soluble in all proportions with a given solvent, this property is known as miscibility.
Solubility ranges widely from infinitely soluble to poorly soluble; in a relevant sense scientists refer to substances as being soluble, slightly soluble, or insoluble
Insoluble is often applied to poorly soluble compounds, though strictly speaking there are very few cases where there is absolutely no material dissolved

5. Predict the relative solubility in the following cases:
Bromine in benzene and in water
KCl in carbon tetrachloride and in liquid ammonia
formaldehyde (CH2O) in carbon disulfide and in water

6. Solubility Units

8. Solubility Curve shows the temperature dependence on the solubility of a substance

9. Are the solutions the same? How can we describe them?

10. Concentrated contains greater amount of solute per volume of solution
Concentration is the amount of solute present for a given amount of solvent or solution; relative or absolute
Concentrated contains greater amount of solute per volume of solution
Dilute contains relatively small amounts of solute per volume of solution
Add solvent

11. Concentration Units moles of solute M = molarity = liters of solution
ppm = parts per million =
mg of solute
liters of solution

12. Examples
Calculate the molarity of a 1.75 L solution containing 3.45 moles of calcium chloride.
Calculate the molarity of an 855 mL solution containing 2.75 moles of sodium nitrate.

13. A 100. 5 mL IV solution contains 5. 10 g of glucose
A mL IV solution contains 5.10 g of glucose. What is the molarity of this solution?
How many moles of sodium nitrate are in 655 mL of a 3.45 M solution?

14. 150 mL of an aqueous sodium chloride solution contains 0
150 mL of an aqueous sodium chloride solution contains g of sodium chloride. Calculate the concentration of sodium chloride in parts per million.
If 25 grams of a chemical is dissolved in 75 grams of water, what is the concentration of the chemical in parts per million?

15. Heat solvent to dissolve excess solute then cool down
Saturation the state that occurs when no more of something can be absorbed, combined, or added
Unsaturated
Saturated
Supersaturated
Add more solute
Heat solvent to dissolve excess solute then cool down

16. A saturated solution contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature.
An unsaturated solution contains less solute than the solvent has the capacity to dissolve at a specific temperature.
A supersaturated solution contains more solute than is present in a saturated solution at a specific temperature.

17. Crystallization is the process in which dissolved solute comes out of solution and forms crystals; describes the separation of excess solid substance from a supersaturated solution.
Sodium acetate crystals rapidly form when a seed crystal is
added to a supersaturated solution of sodium acetate.

18. Factors that Affect Solubility
Temperature
Solids
Gases
Pressure (gasses only)

19. Solid Solubility & Temp
Sugar
Salt

20. Solid/liquids

21. Gas Solubility & Temp

22. Gas Solubility & Pressure

25. Henry’s Law
The solubility of a gas in a liquid is proportional to the pressure of the gas over the solution
S is the solubility of the substance in solution
𝑆 1 𝑃 1 = 𝑆 2 𝑃 2
P is the pressure of the gas over the solution
low P
high P
low c
high c

26. Example
The solubility of a gas is 0.35 g/L at 25.0 kPa of pressure. What is the solubility when the pressure is increased to 115 kPa?