Ch.5 Concentration

Concentration

Amount of solute per the amount of solution

Solubility

Whether a substance will dissolve in a solute

When solids increase in temp

It increases in solubility

Pressure has no effect on

A solid’s solubility

A decrease in temp for gases means

An increase in solubility

For gas, an increase in pressure means

An increase in solubility

Saturated

The solute has been dissolved to the limit

Unsaturated

The solute has been dissolved lower than the limit

What happens if you add more solute to a saturated solution?

The extra solute will dissolve to the bottom

What happens if you add more solute to an unsaturated solution?

The extra solute will dissolve

Hydrophobic

Water fearing and can not hydrogen bond

Hydrophilic

Water loving and can hydrogen bonding

concentration equation

Amount of Solute (g)/ Amount of Solution (mL)

Molarity

Number of moles of solute in a solution

Molarity equation

Molarity (M)=Moles of solute/1 L of solution

1 mole =

The atomic number of an element

Molar mass =

1 mole of a substance

What is the Molar mass of Nitrogen?

14.01 g/mol

Molarity equation 2

Mole/L

Dilution

The process of adding water to reduce solute concentration

During dilution, the number of moles or amount of solute is

Constant

Higher concentration units

C1 Concetration, V1 Volume

Dilution equation

C1 x V1= C2 x V2

Osmosis

Net movement of water through a semipermeable membrane

Isotonic

Equal concentration to blood cells

Hypertonic

Higher solute concentration then blood cells

Hypotonic

Lower solute concentration than blood cells

Equivalent

The amount of any ion that has the same total charge of 1 mole of hydrogen ions.

The number of equivalents is

Equal to the number of charges

Equivalent equation

Mole (element) x Eq (Element)/Mole (element)