Transcript Document
UNIT 8, PART I - SOLUTIONS AND SOLUBILITY
KEY TERMS
Anion - A negatively charged ion
Aqueous Solution - A solution where water is mixed with something to make a solvent
Cation - A positively charged ion
Concentration - The amount of solute per unit volume of solution
Dilution - Weakening or reducing the concentration
Molarity (M) - Concentration measured by the number of moles of solute per liter of solution
Insoluble - Incapable of being dissolved
Polarity - A separation of electric charge leading to a molecule having an electric dipole
Saturated Solution - A solution that contains the maximum amount of solute at a given
temperature
KEY TERMS
Solubility - The quantity of a particular substance that can dissolve in a particular solvent
Solubility Curve - A graph showing the relationship between solubility and temperature
Soluble - Able to be dissolved
Solute - The dissolved matter in a solution
Solvent - Able to dissolve other substances
Unsaturated Solution - A solution that contains less than the maximum amount of
solute at a given temperature
WATER AS A SOLVENT
Water is the most effective solvent
Water will dissolve many ionic compounds and most
polar covalent compounds
Water is not effective as a solvent for non-polar
covalent compounds
Effectiveness of water is because water is highly polar
with hydrogen bonds
Used courtesy of: http://www.volusia.org/services/public-works/water-resources-and-utilities/
WATER AS A SOLVENT – POLARITY (IT IS THE KEY)
Image used courtesy of: http://www.ecfs.org/projects/prepole/MARINE%20BIOLOGY%2012/Chapter%20Readings/Ch%201%20Oceanography/Chapter%201%20Notes.htm
WATER AS A SOLVENT- HYDROGEN BONDING
The powerful attraction between
an oxygen atom from one water
molecule and a hydrogen atom
from another water molecule
Image used courtesy of CINCH ® Learning
Image used courtesy of: http://www.glogster.com/arooke2/hydrogen-bonds/g-6m99vd692fc7hgidt985ta0?old_view=True
SOLUBILITY
The ability to dissolve a solute in a solvent to form a
solution, a homogeneous mixture
Solute – The matter dissolved in a solvent
Solvent – The matter in which a solute is dissolved
Solution – Homogeneous mixture
TYPES OF SOLUTIONS
FACTORS AFFECTING SOLUBILITY
It is all about polarity!!
The nature of the solvent affects solubility
Like Dissolves Like
Ionic compounds, if they are soluble, dissolve in polar solvents
Polar molecular (covalent) compounds dissolve in polar solvents
Non-polar molecular (covalent) compounds dissolve in non-polar solvents
FACTORS AFFECTING SOLUBILITY
Factors affecting the solubility of solids and liquids
Temperature
Generally, as temperature increases, the solubility of solids and liquids increases
Factors affecting the solubility of gases
Temperature
Generally, as temperature increases, the solubility of gases decreases
Pressure
Generally, as pressure increases, the solubility of gases increases
SUMMARY OF FACTORS AFFECTING SOLUBILITY
Temperature
As temperature ↑, solubility of liquids and solids↑
As temperature ↑, solubility of gases↓
Pressure
As pressure ↑, solubility of liquids and solids is unaffected
As pressure ↑, solubility of gases ↑
SUMMARY OF FACTORS AFFECTING SOLUBILITY
Nature of Solvent
Generally the nature of the solvent will determine what kinds of matter
will dissolve in it.
Polar solvents (such as water) will generally dissolve polar compounds.
Non‐polar compounds will generally dissolve non‐polar compounds.
Ionic compounds, if they are soluble, dissolve in polar solvents
Polar molecular (covalent) compounds dissolve in polar solvents
Non‐polar molecular (covalent) compounds dissolve in non‐polar solvents
LIKE DISSOLVES LIKE!
CONCENTRATION AND SOLUBILITY
The amount of solute affects both solubility and
dissolving rate.
A solvent can only dissolve so much solute.
As the concentration increases, the ability to dissolve
more decreases
DISSOLVING RATE
The rate at which the solute dissolves in the solvent
As Kinetic Energy increases, dissolving rate increases
As Kinetic Energy decreases, dissolving rate decreases
As the number of collisions increases, dissolving rate increases
As the number of collisions decreases, dissolving rate decreases
DISSOLVING RATE
Factors affecting dissolving rate
Temperature
As temperature increases, dissolving rate increases
Surface Area
As surface area increases, particle size decreases
As surface area increases, dissolving rate increases
Agitation
As agitation increases, dissolving rate increases
TEMPERATURE AND DISSOLVING RATE
Since temperature is a measurement of the average kinetic energy, changing the temperature by
adding or removing heat will change the rate of dissolving.
Increasing the temperature speeds up the movement of its particles
The change in temperature will affect both the number of collisions and the probability that as
particles collide the solute will dissolve in the solvent.
Allows for more collisions between solute particles and solvent particles
Used courtesy of: http://www.seriouseats.com/2012/10/ask-the-food-lab-on-hot-chocolate-and-whole-wheat.html
SURFACE AREA AND DISSOLVING RATE
Breaking a solid into smaller pieces greatly increases its surface area
More solvent particles can come into contact with more particles of the solute
corresponding to increased surface area
Rate of collisions increases as surface area increases
AGITATION AND DISSOLVING RATE
Agitation is the result of an external force causing the motion of the solute
and the solvent such that there is an increased chance of collision.
Stirring, Mixing, Shaking
As agitation speed increases, rate of dissolving increases
As the solvent moves around, more collisions occur between solvent and
solute particles
Used courtesy of: http://www.pennlive.com/lehighvalley-generalent/index.ssf/2008/06/in_defense_of_koolaid.html
SUMMARY OF FACTORS AFFECTING DISSOLVING RATES
As temperature ↑, dissolving rate ↑
As particle size ↓, surface area↑, dissolving rate ↑
As agitation ↑, dissolving rate ↑
CONCENTRATION AND SOLUBILITY
The amount of solute affects both solubility and dissolving rate.
A solvent can only dissolve so much solute.
As the concentration increases, the rate at which it will dissolve
decreases.
CONCENTRATION OF SOLUTIONS
Concentration – the degree to which a solution contains the maximum
amount of solute.
Directly related to density
Qualitative
Uses terms saturated and unsaturated to reference the amount of solute
dissolved in the solvent
Quantitative
Molarity – the number of moles dissolved in one liter of solution
SOLUTIONS AND SATURATION
• Saturated Solution – A solution is considered saturated when it contains the maximum
amount of solute given the volume and environmental conditions of the solvent.
• Unsaturated Solution – Any solution into which more solute can be dissolved is unsaturated.
• An unsaturated solution that is close to the point of saturation is referred to as
“concentrated”.
• An unsaturated solution well below the point of saturation is referred to as “dilute”.
• Super‐Saturated Solution – Any solution that contains more dissolved solute than it could
contain under normal conditions is super‐saturated.
• A beverage with carbonated water is a supersaturated solution. It is packaged into cans or
bottles under conditions of high pressure. When the can or bottle is later opened, the carbon
dioxide bubbles out of solution under the lower pressure.
• Rock candy is made using a supersaturated solution of sugar and allowing the sugar crystals
to slowly form on a string dipped in sugar.
SOLUTIONS & SATURATION
Unsaturated
Saturated
Supersaturated
Definition
Contains less than the
maximum amount of solute.
More solute can dissolve in
the solvent
Contains the maximum amount of
solute. No more solute will dissolve
in the solvent. If there is extra
undissolved solute, it will settle to
the bottom of the container.
Contains more
dissolved solute
than the maximum
under normal
conditions
Solubility Curve
Below the saturation line
On the saturation line
Above the
saturation line
Can you Dissolve
More Solute?
Yes
No
No, it is already past
saturation point
Imaged used courtesy of: http://www.mts.net/~alou/Chemistry%2011/Unit%204%20-%20Solutions%20Lessons/Lesson%203%20-%20Factors%20Affecting%20Solubility.htm
SOLUBILITY CURVES
Show the amount of solute that can dissolve in a solvent under normal
circumstances at a given temperature
The line for a given element on a set of solubility curves is called the saturation
line
Comparisons are made using the line for a given compound
Under the curve – the solution is unsaturated
Above the curve without excess – the solution is supersaturated
Above the curve with excess – the solution is saturated
On the curve – the solution is saturated
SOLUBILITY CURVES
QUANTITATIVE SOLUBILITY: MOLARITY
Measured as moles of solute per liter of solution
Molarity = Moles of solute
Liters of solution
M = Moles
Liter
MOLARITY EXAMPLE
116.88 grams of NaCl are dissolved in 1.5 liters of solution. What is the molarity of this solution?
First, convert grams of NaCl to moles NaCl
Found by dividing 116.88g by the molar mass of NaCl, 58.44 g/mol
116.88g NaCl is 2.00 moles of NaCl
Next, divide moles solute by liters of solution
2.00 moles NaCl = 1.33 mol NaCl/L = 1.33 M NaCl
1.5 L
DILUTION
What does it mean to dilute a solution?
Solutions can be diluted simply by adding water and leaving the amount of solute unchanged
What happens to molarity when a solution is diluted?
More water has been added, so the total volume of solution is greater but the amount of solute is the same
Molarity will decrease!
We use the following equation to perform dilution calculations:
M1V1=M2V2
M1=Initial molarity
V1= Initial volume
M2= Final molarity
V2=Final volume
DILUTION EXAMPLE
What would be the resulting molarity of 2.5 L solution when the starting solution had a molarity
of 6.00 M and a volume of 417 mL?
M1= 6.00 mol/L
V1= 417 mL
M1V1=M2V2
(6.00 mol/L)(417 mL) = (M2)(2500 mL)
(M2) = (6.00 mol/L)(417 mL)
(2500 mL)
M2 = 1.00 mol/L
M2= ??
V2= 2500 mL
DISSOCIATION AND DISPERSION
Dissociation – When ionic compounds dissolve, they separate into the ions that were bonded together.
Example: Potassium sulfate will dissociate into potassium ions and sulfate ions.
K2SO4 → 2K1+ + SO42 More examples of dissociation:
NaCl → Na1+ + Cl 1 MgCl2 → Mg2+ + 2 Cl1 Al2(SO4)3 → 2 Al3+ + 3SO42-
Dispersion – When complete dispersion occurs, the molecules of the solute are uniformly mixed with the
molecules of the solvent.
This occurs with covalent compounds.
ELECTROLYTIC SOLUTIONS
Electrolytic solutions conduct an electrical current
Ions dissociate when dissolved in water
Ions, because they are charged particles, act as a path for the flow of electricity
The more ions present, the more electrolytic the solution is
Non-electrolytic solutions do not conduct an electrical current
ELECTROLYTIC SOLUTIONS
Electrolyte
Soluble Ionic
Solute
Non-Soluble Ionic
Solute
Non-Soluble
Covalent
Solute
Yes
No
No
CONTROLLING ELECTROLYTIC SOLUTIONS
In order to increase the electrolytic properties of a solution you must increase the concentration of ions present
in the solution
Reduce the volume of the solution while maintaining the amount of electrolytic solute
Increase the amount of electrolytic solute without modifying the volume
Using a different electrolytic solute which produces more ions when it dissociates
In order to decrease the electrolytic properties of a solution you must decrease the concentration of ions
present in the solution
Dilute the electrolytic solution
Using a different electrolytic solute which produces less ions when it dissociates