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Define the following vocab: Solution -Solubility Solute -Saturated Solution Solvent -Unsaturated Solution Soluble -Supersaturated Solution Insoluble -Electrolyte Miscible -Non-Electrolyte Immiscible -Solvation (draw f/pg455)

Solutions

Factors that Affect Solubility Temperature and Pressure Affect Solubility For Solids and liquids being dissolved As temperature increases solubility increases (more will dissolve)   For gases being dissolved As temperature decreases and pressure increases, solubility of the gas increases (more will dissolve)

Concentration VS Dilute Solutions Concentrated: Large amount of solute in a small amount of solvent (you must have a solute and solvent to have a solution) Dilute: Small amount of solute in a large amount of solvent

Molarity Molarity= Moles of solute/Liters of solution   Example: What is the molarity of the solution of 45g of NaCl dissolved in 500mL of solution? 45g x 1 mole/ 58.44g = 0.77 mol 500mL/1000mL = 0.500 L Molarity= 0.77/0.500= 1.54M

Molality Molality= Moles of solute/ Kilograms of solvent   Example: What is the molality of a solution of 65g of CO2 dissolved in 750g of water? 65g x 1 mole/ 44.01g = 1.48 mol 750g/ 1000g= 0.750 kg Molality= 1.48/0.750 = 1.97m

Molarity by Dilution This equation is used every time that we want to make a solution for students to use in a lab! M1 x V1 = M2 x V2   M1= Molarity of the concentrated liquid V1= Volume (amount) of the concentrated liquid needed to make the solution M2= Molarity of the diluted solution you are wanting to make V2= Volume (amount) of the diluted solution you are wanting to make

Molarity by Dilution Example: What volume of a 20M HCl solution is needed to make 500mL of a 2M HCl solution? 20M x V1 = 2M x 500mL V1 = (2M x 500mL) / 20M V1 = 50mL

Molarity by Dilution How much water is needed to make the dilute solution? Water needed= (V2) –(V1) Water needed = 500mL – 50mL Water needed = 450mL