Unit 4 Part 2Solutions

Components of a Solution

A solution is composed of two or more pure substances, one of which is a solvent and the other a solute.

Components of a SolutionA cup of instant coffee is the

____________, the hot water is the ____________, and the instant coffee is the ____________.

Solvent Solution Solute

Components of a Solution Solutions in which water is the solvent

are called aqueous solutions.

Water as a SolventMost covalent liquids are only

able to dissolve other covalent compounds; water can dissolve both ionic and covalent compounds.

Water as a solvent

Water as a solventThe attraction of water

dipoles for ions pulls ions out of a crystalline lattice and into aqueous solution.

 Solutions: A saturated solution is a solution that

contains the maximum amount of solute dissolved in a solvent. A supersaturated solution is a solution where conditions have been changed to allow more solute to dissolve than would at room temperature (this is done by heating the solvent or solution).

Solutions: When the solvent and solutes are liquids

we can use the terms miscible and immiscible. Miscible means that the two liquids will mix together, and immiscible means that the two liquids will not dissolve in one another.

Solutions: Sometimes when we mix two dissolved

salts together, we end up with a precipitate. This is because a new ionic compound is formed that is insoluble in water.

Solutions: We can use solubility charts or solubility tables

to determine if a solid will be formed.Ion Solubility ExceptionsNO3

– soluble none

ClO4– soluble none

Cl– soluble  except Ag+, Hg22+,

*Pb2+

I– soluble except Ag+, Hg22+,

*Pb2+

SO42- soluble except Ca2+, Ba2+, Sr2+,

Hg2+, Pb2+, Ag+ CO3

2- insoluble except Group IA and NH4

+

PO43- insoluble except Group IA and

NH4+

OH– insoluble except Group IA, *Ca2+, Ba2+, Sr2+

S2- insoluble except Group IA, IIA and NH4

+

Na+ soluble noneK+ soluble noneNH4

+ soluble none

Solutions Ex. If we mix sodium ions with

hydroxide ions will a precipitate form?

Ex. If we dissolved sodium hydroxide in calcium chloride, will a precipitate form?

2NaOH + CaCl2 2NaCl + Ca(OH)2

Solutions Ex. Calcium nitrate with sodium

carbonate Ca(NO3)2 + Na2CO3 CaCO3 + 2NaNO3

Ex. Silver Perchlorate and Calcium Iodide

Ca(ClO4)2 (________) and AgI (__________)

DemonstrationsIon Solubility Exceptions

NO3– soluble none

ClO4– soluble none

Cl– soluble  except Ag+, Hg22+, *Pb2+

I– soluble except Ag+, Hg22+, *Pb2+

SO42- soluble except Ca2+, Ba2+, Sr2+,

Hg2+, Pb2+, Ag+

CO32- insoluble except Group IA and

NH4+

PO43- insoluble except Group IA and

NH4+

OH– insoluble except Group IA, *Ca2+, Ba2+, Sr2+

S2- insoluble except Group IA, IIA and NH4

+

Na+ soluble noneK+ soluble none

NH4+ soluble none