Chemistry Honors - Unit 9 Solutions.

Solvent

Dissolving medium of a solution.

Solute

Dissolved particles of a solution.

Solvation

Ion capture by the solvent.

Aqueous Solution

A solution where water is the solvent.

Aqueous Solution Equation

Solute + Solvent = Solution.

Electrolyte

A compound that conducts electric current when dissolved in an aqueous solution or molten state.

Nonelectrolyte

A compound that does not conduct electric current in either an aqueous solution or molten state.

Dissolution Rate.

The rate at which a solute dissolves.

3 factors that affect dissolution rate

Adding heat, increasing motion and changing particle size.

Saturated Solution.

Maximum amount of solute for a given quantity of solvent at constant temperature.

Solubility

A substance is the amount of solute that dissolves in a given quantity of a solvent at specific temperature and pressure to produce a saturated solution.

Unsaturated Solution

Can dissolve more amount of solute for a given quantity of solvent.

Solubility Curve

A graph of the solubility as function of a temperature.

Solubility of Gases

Solubility decreases with increasing temperature.

Supersaturated Solution

Contains more solute than it can theoretically hold at a given temperature.

Homogeneous Mixture.

Uniform appearance and composition.

Heterogeneous Mixture.

Not uniform in composition and are considered solutions.

Colloid

A heterogeneous mixture containing particles, called dispersed phase, that can spread throughout another mixture, can not be filtered, clumped molecules or ions, 10^-7 - 10^-5 cm, visible, reflect light, can not be filtered.

Suspension.

A heterogeneous mixture from which particles settle out upon standing, large particles, can be filtered, 10^-5 cm and greater.

Tyndall effect

Different types of particles reflect light differently.

Solution

A homogeneous mixture with molecules and ions, less than 10-7 cm, transparent, no reflection of light, can not be filtered.

Concentration

A measure of the amount of solute that is dissolved in a given quantity of a solvent.

Dilute Solution

A solution with a small amount of solute.

Concentrated Solution

A large amount of solute.

Molarity

The number of moles dissolved in Liters of a solution.

Molarity Equation

Molarity = moles of solute/liters of solution.

Dilutions

Reduces the numbers of moles per unit volume but not the total numbers of the solvent does change.

Dilutions Equation

M1V1=M2V2

Percent by Volume

Ratio of the volume of solute to solution.

Percent by Volume Equation

% by Volume = volume of solute/volume of solution.

Percent by mass

The ratio of the masses of solute and solution.

Percent by mass Equation

% by Mass = mass of solute/mass of solution x 100

Compete Ionic Equation

Dissolved ionic compounds s dissoclated free ions.

Spectator Ions

An ion that appears on both sides of an equation and is not directly involved.

Net Ionic Equation

An equation for a reaction in solution that shows only those particles that are involved.

Strength of intermolecular forces

Between water molecules and substance's ions in solution affect the solubility of a substance.

Solvation Shell

A sphere of solvent particles that surround a solute.

Substances formation of precipitation

Insoluble Solvent.

Rule #1 of Solubility Rules

Nitrate (NO3^-) salts are soluble.

Rule #2 of Solubility Rules

Salts containing alkail metal ions (Li, Na, K, Rb, Cs and NH4+) are soluble

Rule #3 of Solubility Rules

Most chloride, bromide, and iodide are soluble. Expect for salts containing Ag, Pb, Hg

Rule #4 of Solubility Rules

Most sulfate are soluble. Expect for BaSO4, PbSO4, Hg2SO4, and CaSO4

Rule #5 of Solubility Rules

Hydroxide salts are soluble. But if there's more than one, it will be insoluble.

Rule #6 of Solubility Rules

Sulfide, Carbonate, Chromate, and Phosphates are insoluble.