1. Are homogeneous mixtures that come in solid, liquid, or gaseous form.
Solutions
Are homogeneous mixtures that come in solid, liquid, or gaseous form.
Solute
Solvent

2. Factors Affecting Solubility
Nature of the solute and the solvent
Agitation
Temperature
Size of particles/Surface Area

3. What is solubility? Ability to get dissolved or to be dissolved
Is the amount of solute dissolved in a given amount of solvent at specified conditions of T and P to produce a saturated solution.

4. Types of solution in terms of concentration
Saturated Solution – contains the maximum amount of solute for a given amount of solvent at a constant T.
Unsaturated Solution – contains less amount of solute than a saturated solution.
Supersaturated Solution - contains more solute than a saturated solution.

5. Ways of Expressing Concentrations of Solutions
1. Molarity/Molar Concentration – is the number of moles of solute per 1L of solution.
M = n of solute / L of solution
2. Dilution – means adding more solvent to the concentrated solution.
M1V1 = M2V2
3. Percent Solutions by volume– when both solute and solvent are liquids
% V = Volume of solute / Volume of solution x 100%
% Mass = mass of solute / mass of solution x 100%
Molality (m)/Molal Concentration = moles of solute/ kg of solvent
Mole Fraction = mol of solute / mol of solution

6. Molarity Problems (M = moles of solute / liters of solvent)
A salt solution has a volume of 250mL and contains 0.70mol of NaCl. What is the molarity of the solution?
A saline solution contains 0.87g of NaCl per 50.0 mL of solution. What is the molarity of the solution?
 How many grams of solute are present in 1.5L of 0.20 M Na2SO4?
Calculate the molarity of the ff:
a mol of KCl in 750mL of solution.
400g of CuSO4 in 4.00 L of solution.
5.  How many moles of solute are in 250mL of 2.0M CaCl2? How many grams of CaCl2 are there?