Module 11A- Solutions 1

solution

Homogeneous mixture of two or more substances

Solute

Substance present in smaller amount in a solution

Solvent

Substance present in greater amount in a solution

Concentration

Amount of solute contained in a given amount of solvent or solution

Solubility

Maximum amount of a solute which can be dissolved in a given amount of solvent or solution

Unsaturated solution—-

More solute can dissolve

Saturated solution—-

Contains as much solute as possible at a particular temperature and pressure

• Solution will have undissovled clumps

Supersaturated solution—-

Contains more so youth than it normally can out of a particular temperature due to a heating and cooling down process

Electrolyte

Substance which breaks into ions when dissolved in water. The resulting solution conduct electric electricity when voltage is applied to it.

Strong electrolytes

breaks in 100% ions

We electrolytes

Break up into 5-10% ions

Not electrolytes

breaks into 0% ion

6 common strong acids

Hydrochloric acid, hydroidic acid, sulfuric acid, hydrobromic acid, nitric acid, perchloric acid

Common non-electrolytes

Urea (NH2CONH2) and glucose (C6H12O6)

9 strong bases

LiOH, NaOH, KOH, RbOH, CsOH, FrOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Molarity

moles solute/ Liters solution

Mole fraction (X)

moles of component/ total moles

Weight or mass percent

(grams of solute/ total or solution grams) *100%

Molality

moles solute/kg solvent

What three factors affect solubility?

Temperature, pressure, and nature of the solute and solvent

How does temperature affect solubility for solids and gases in water?

Solids: directionally proportional

Gasses: inversily proportional

How does pressure affect solubility for solids and gases in water?

Gases: directly proportioal

solid/liquids: pressure has little effect