Solubility and Saturation Flashcards
soluble
more than 1g of solute dissolves in 100 mL of solvent at room temperature
insoluble
less than 1g of solute dissolves in 100 mL of solvent at room temperature
what affects solutbility?
- molecule size
- ion charge and size
- temperature
- pressure
solubility
the quantity of solute that can dissolve in a gien quantity of solvent at a given temperature
how is solubility expressed?
as a maximum mass of solute that can be dissolved per 100g of solvent at a given temperature.
How does molecule size affect the solutbility of a covalent substance?
small molecules are often more soluble that larger molecules
most alkali metal compounds are soluble in water
solfide and phosphates are usually insoluble in water
How does the ion charge affect solubility?
soluble
smaller the ionic charge the more soluble a substance is, the larger the ionic charge the greater the force that holds ions together.
small ion charge = soluble
large ion charge = insoluble
smaller the ion NOT CHARGE, the stronger the force. compounds with small ions tend to be less soluble than those with large ions Why?
small ions bond more closely together than large ions, bunds between small ions is stronger than bond between large ions with same charge
How does temperature impact the solubility of solids?
solubility increases with temeperature, higher temperature means more energy to break the bonds
How does temperature impact the solubility of liquids?
not greatly affected by temperature, addtional energy to break bonds not needed
How does temperature impact the solubility of gases?
solubility of gases descreases with higher temperature
how to changes in pressure affect solubility for liquids and solids?
JK They don’t
How does pressure impact solubility of a gas
directly proportional to the pressure of gas above the liquid
think of pop bottle opening
How does high pressure work wit gases?
when the gas is compressed, gas molecules enter the liquid more frequently so more are dissolved
Diver + pressure
- pressure increases the deeper you go
- increased pressure causes the nitrogen in lungs to dissolve into the blood
- as diver surfaces gas comes out of solution
of surfaces too quixkly, can form bubbles in the blood
saturated solution
a solution that contains the maximum quantity of solute at a given temperature
unsaturated solution
a solution that contains less than the maximum quantity of solute
supersaturated solution
force a solution to dissolve more solute than it normally would at a given temperature and pressure
How do you achieve a supersaturated solution?
achieved by heating a solutionn, saturating it at a higher temperature then allowing it to cool.
solubility curves of gases
GO DOWNNNNNN
gas particles have a lot of kinetic energy, when gas dissolves loses some of this energy, at higher temps the dissolved gas gains energy again and the gas comes out of the solution
concentration definition
the ratio of the quantity of solute to the quantity of solution
dilute solution
has a relatively small quantity of solute per unit volume of solution
concentrated solution
has a relatively large quantity of solute per unit volume of solution
2 ways a concentration of solution can be expressed
- amount concentration (molar concentration)
- percentage concentration
amount concentration, molar concentration
expressed in units of mol/L
old version
uses molarity
percentage concentration 3 ways:
volume by volume
mass by volume
mass by mass (
when is percentage volume by volume often used?
liquid in liquid solution
(v/v)
when is percentage mass by volume most often used?
when a solid solute is dissolved in a liquid solvent (usually g/mL) (m/v)
when is percentage mass per mass often used?
when a solid solute is dissolved in a solid solvent (m/m)
parts per million (ppm)
1 part per million parts solution - 1: 10^6
parts per billion (ppb)
1 part per billion parts solution - 1: 10^9
parts per trillion(ppt)
1 part per trillion parts solution - 1: 10^12
ppm, ppb, and ppt are
(m/m) ratios
