Test on solutions Flashcards
Solution
Homogenous mixture of two or more substances physically mixed together
Solute
substances that get dissolved in solution.
Example, salt in water
Solvent
Substance in a solution that does the dissolving.
Example, water dissoving salt
Electrolyte (type of solute)
Ionic compounds (metals + Non-metal)
A chemical compound that conducts electricity by changing into ions when melted or dissolved in a solution.
Strong electrolyte
-strong electrolytes: soluble ionic compounds
Dissociate completely in water (only ions)
Example, NaCl (ionic compound) in water seperates completly to only ions. creating a homogenous miixture.
Weak electrolytes (only ions)
Weak Electrolyte
“Insoluble” ionic compounds
Only partially seperates in aqueous solutions.
Example, AgCl in water. only partilly seperates
some AgCl stay together
(few ions)
NonElectrolytes
Covalent or molecular compounds (non metals)
NO IONS!!
Example:
Ch3OH
Does not dissolve in water
Solubility
The ability of a substance (solute) to dissolve in another substance is called Solubilty.
Insoluble
When a substance doesnt dissolve in another substance.
Miscible meaning
Soluble
(used mostly for liquids dissolved in other liquids)
How to do solvents work?
What causes them to dissolve?
Likes dissolve likes
(Based on IMF’s)
Example, CH4 and N2
Saturated solution
A solution that has the solute and solvent in dynamic equilibrium
**it holds the maximum amount of solute**
(if you add more solute, it will not dissolve)
example, for NaCl at 20* C 35g/100g is a saturated solution
Unsaturated solution
A solution that has less solute than saturation
Super Saturated
A solution that contains more solute than Saturation
Molarity formula (M)
=moles solute
L solution
Converion factor
M=m/L
