Solutions Flashcards
Solution
Homogenous mixture
Solute
Substance being dissolved
Solvent
Present in greater amount, in what solute is being dissolved
Molarity
A way to describe concentration of a solution used in the lab
Number of moles dissolved in each liter of solution
Molarity formula
Moles/ liters
M= n/L
M=n/v
N=MV
Diluting formula
MV=MV
Solvation
The process of dissolving
What are needs for dissolving/ solvating
Needs to be enough solvent and enough energy
When solute particles are surrounded by solvent particles…
Needs to be enough solvent
When solute particles are separated and pulled into solution…
Need to be enough energy
How does dissolving happen with characteristic of solute and solvent (polarity)
Like dissolved like
Except ionic dissolved in polar
Seeding
Putting crystal in
Unsaturated
More solute dissolves
Crystal will dissolve
Saturated
No more solute dissolves
Crystal falls to the bottom
Super saturated
Becomes unstable
Crystal forms
Crystal will fall with more than it had put in
What is the relationship with concentration from unsaturated to saturated
Increases
Stronger solvent when add
Heat energy
Solubility
Maximum grams of solute that will dissolve in 100g of solvent at given temp
Solubility curve
Shows the dependence of solubility on temperature
Solubility curves
Below
On line
Below- unsaturated
On line- saturated
On solubility curve Over line is
Supersaturated if
Put it in saturated with some on bottom, if heated up and dissolve and cooled down then supersaturated
Gases solubility
Low temps High pressure (Henry law) a
Solids solubility
Solids are more solvable at high temps
Colligative property
Property that depends on the concentration of the solute particles, not their identity
