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terms: saturated solution, solubility, unsaturated solution, miscible, immiscible, concentration, dilute solution, concentrated solution, molarity, colligative properties, boiling point elevation, freezing-point depression, molality, mole fraction

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Chapter 18 - Solutions

18.1 Properties of Solutions

Solution Formation Solvent

This is the liquid that is doing the dissolving Solute

This is what is being dissolvedForm a homogenous mixture

Solubility

When a solute is dissolved, an equilibrium is established: Equilibrium is a condition in which both

reactants and products are present in concentrations which have no further tendency to change with time

EXAMPLE:HC2H2O3 ↔ C2H3O2

- + H+

Solubility

When an equilibrium is established, the solution is said to be saturated

If a solution is not at equilibrium, then it is said to be unsaturated (solution has the ability to hold more)

Saturated vs. Unsaturated Solutions

Solubility

Two liquids that dissolve in each other are said to be miscible

Immiscible liquids are insoluble in each other

Immiscible vs. Miscible Solutions

Factors Affecting Solubility

Solubility increases with the increase in temperature (Easier to dissolve something when the temperature is increased)

Solubility increases with an increase in surface area (ex. CRUSHING) Few exceptions that occur in the reverse

Thursday, April 10th, 2014

PDN: What is the differences between miscible and immiscible? Saturated and unsaturated?

Daily Log: Molarity Notes Molarity Calculations

18.2 Concentrations of Solutions

Molarity is the concentration of moles per liters Molarity (M) = moles of solute / liters of

solution Dilute solution contains a low concentration

of solute Concentrated solution contains a high

concentration of solute

Practice Problems:

Calculate the molarity of a solution which contains 0.40 mol of C6H12O6 dissolved in 1.6 L of a solution.

What is the molarity of a solution containing 325 g of NaCl dissolved in 750. mL of solution?(1000 ml = 1L)

Monday, April 14th, 2014

PDN: Determine the volume of a 1.7M solution containing 3.3 grams of NaCl.

Daily Log: Science Scheduling Dilution Notes/Practice Problems

Making Dilutions

Formula for making a dilution C1 X V1 = C2 X V2

“Stock solution” is the same as the original solution.

Example

A stock solution of HCl has a concentration of 12M. How much of the stock solution would be required to make 325 mL of a 6M solution?

Monday, April 21st, 2014

Daily Log: Molality Notes Practice Problems Chapter 18 Test on

Friday

Molality

Molality is another way to represent the concentration of a solution.

It is represented by a lower case m. Molality = moles of solute/kg of solvent

Example: A 4.9m solution of NaCl is dissolved in 1000 grams of water. How many grams of NaCl is this?

Tuesday, April 22nd, 2014

PDN: Determine the molality of a NaCl solution in which 17.3 moles of solute are dissolved in 1400 grams.

Daily Log: Practice Problems Test on Friday!

18.3 Colligative Properties of Solutions

Properties that depend on the number of particles dissolved in a given mass of solvent Boiling Point Elevation Freezing Point Depression

Boiling-Point Elevation

∆Tb = Kb x m x im is the molaityi is the number of ions in solution

Kb is the molal boiling point elevation constantIt is dependent on the solvent

Freezing Point Depression

∆Tf = Kf x m x im is the molaityi is the number of ions in solution Kf is the molal freezing point constantIt is also dependent on the solvent

Example:

Determine the boiling point and freezing point of a solution in which 600 grams of MgCl2 is dissolved in 2400 grams of water. (Kb = 0.512 and Kf = 1.86)