Chemistry 12: Solubility Equilibrium

Dissociation Equations

Refers to the equation representing the dissociation of an ionic compound into component ions upon mixing with water

Anhydrous

Dry

Reference Values

Do not determine significant figures, only measured numbers

Dilution Calculations

M1V1=M2V2, must solve for variable before the insertion of numbers

Dimensional Analysis

The converting from one dimension unit to another

Water

Cannot break down molecules which are covalently bonded

Electrolyte

Ionic solution that conducts electricity

Non-Electrolyte

Molecular solution that does not conduct electricity

Solutions

Homogeneous mixture of 2 or more pure substances

Solvent

Component in greater proportion

Unsaturated

When a solution is capable of dissolving more solute

Saturated Solution

When a solution is no longer capable of dissolving added solute, only a fixed amount of solute will dissolve in a given volume of solvent

Solubility

The amount of substance needed to make a saturated solution at a given temperature

Miscibility

2 liquids are completely soluble in one another regardless of proportion, ex. alcohol and water

Immiscible

Substance that will not mix, and instead form 2 distinct layers, ex. oil and water

Alloy

Solid with solid solution

Water

Universal solvent, polar molecule, dipole will align itself to other polar substances

Dissociation

When the solute upon contact with solvent breaks apart into component ions, which is the process of forming ions, often spontaneous and exothermic

Salt Water

The polar ends of water molecules provides sufficient force to pull Cl- and Na+ away from the salt crystal resulting in free flowing ions in a solution

Rule of Thumb

"like dissolves like"

Ethanol and Water

Both are polar and will be attracted to oppositely charged poles of neighbouring molecules (solvation), due to this attraction mixture will occupy smaller volume

Oil and Vinegar

Oil is non-polar and vinegar which is mostly water, is polar, since oil molecules have no dipole, they feel very attraction to vinegar molecules

Density

Non-polar and polar separate according to density, less dense substance floats

Ionic Solutions

Dissolving and dissociation, will conduct electricity

Molecular Solutions

Dissolves but does not dissociate, will not conduct electricity, tend to be covalently bonded compounds

Dissolving

When two or more pure substances mix to form a homogeneous mixture

Insoluble

Unable to dissolve to any extent, (not entirely true because all solutes dissolve to some extent)

Low Solubility

Amount of dissolved solute is extremely small but cannot be neglected

Soluble

Amount of dissolved salt is appreciable

No Reaction

If both products are soluble

Hard Water

Water containing significant amounts of Ca+2 and or Mg+2

Origin of Hard Water

Acid rain or natural acid deposits react and dissolve CaCO3 and MgCO3 from limestone and rock containing these minerals

Impacts of Hard Water

Bitter taste, white deposits of CaCO3/MgCO3 when water evaporates or is heated , and inhibits cleaning action of soaps because it reacts with stearate ion and precipitates calcium/magnesium stearate

Permanent Hard Water

Ions must be removed via selective precipitation

Temporary Hard Water

Boiling the water will result in the formation of insoluble CaCO3 precipitate

Washing Soda

Adding soluble Na2CO3 to precipitate out CaCO3/MgCO3 from water and remove excess Ca+2 and or Mg+2