Name __________________________________________________ Date ______________ Period _______
Water and Solutions – PAP
Essential Question __________________________________________________________________________
_________________________________________________________________________________________________
Water
The _______________ bond is __________________ (uneven
pull on the _____________________)
Water has a __________________ shape so it’s a _______________
molecule as well
Intermolecular
Forces
Attractions that hold __________________________ together
- determine ________________, ___________________, or _________
Types:
1) London Dispersion Forces - _________________________
(present in _______________ molecules)
2) Dipole-Dipole Forces – present in ___________________
molecules
3) Hydrogen Bonding - ______________________ (present in
molecules with _________ and ________, _________, or ________)
Dipole-Dipole Ex.
Hydrogen Bonding
in Water
- Molecules containing these bonds show ______________
strong ___________________________ to one another – keeps
the molecules ________________________________________
- This is the reason for ________________ being a ____________
at __________________ temperature
- Normally molecules with __________________ masses have
________________ intermolecular forces and therefore are
______________________ - but NOT ______________________
Ice
Most things ________________________ as they cool
Water __________________________ until _________________, then
the _______________________ starts to __________________
- Large, ______________________ rings of ice crystals form
- Increase in __________________, so density _________
- Reason that ice __________________ in water
Essential Question __________________________________________________________________________
_________________________________________________________________________________________________
Aqueous Solutions
Solute – what is __________________________________________
Water is the __________________________
- it is doing the _____________________________
Ionic and polar molecules ______________________ in water
Nonpolar molecules __________________
“like ________________________ like”
WHY? Water is ______________________
It has partially __________________ and _________________ ends
Its __________________________ to other __________________
which _____________________________ and other _______________
molecules have
- Water will ________________ anything else with ___________
The __________ of one is attracted to the _________ of other
Water can _______________ ionic compounds apart and
Then _____________________ the ions to _________________ them
Electrolytes
Conducting electricity requires ____________________,
____________________ particles
Ionic compounds that __________________ in water produce
____________________ and are called ___________________________
* Reminder – ions are ___________________ particles
When electricity is passed through the ___________________,
these ______________ carry electricity through the solution
More ______________ means __________________ conductor
Ex. Which is a better conductor: AlCl3 or (NH4)2CO3?
- Most molecular solutions do not split into ____________
and therefore do not ___________________ electricity – they
are called _______________________________
Heterogeneous
Aqueous Mixtures
Suspensions – mixtures that _________________ out upon
standing
- particles are too ________________ to fully dissolve
- they can be ________________
- particles can be _____________________ out
Examples:
Colloids – mixture with __________________-sized particles
- particles are too ________________ to fully dissolve,
but too ___________________ to see
- Look ___________________ or _________________
- Cannot _____________________ out particles
Examples:
Tyndall Effect – both suspensions and colloids
- scattering of ___________________ in all directions
- particles have to be _________________ enough to
reflect ________________
- Solutions ________________ exhibit Tyndall Effect
- particles are too ___________________
Essential Question __________________________________________________________________________
_________________________________________________________________________________________________
Solution Formation
Soluble – substance can _____________________
Ex. Sugar in water
Insoluble – substance __________________ dissolve
Ex. Sand in water
Rate of Solution
Formation
Factors that Increase Rate
1) Stirring/Agitating
- It moves the __________________________________ away
- It brings fresh _________________ in contact with the
_________________ to dissolve more
2) Increasing Temperature
- Increases the _____________________ of the water and
_______________ particles causing them to come in contact
_______________ frequently
3) Increasing Surface Area
- Dissolving takes place from the ____________________
Solubility
Solubility is the _______________________ amount of solute
that can ______________________ in a specific amount of
_______________________ at a specific ___________________________
Types of Solutions
1) Saturated – contains the ______________________ amount
of dissolved ______________________ (can’t dissolve __________
at that ________________________________)
2) Unsaturated – contains _______________ than the
__________________________ amount of _________________
3) Supersaturated – contains ________________ than the
_______________________ amount of ____________________;
- an ________________________ solution
To prepare:
- Add _________________ solute to a ______________________
solution; __________________ it up until the __________________
solute dissolves; let it ______________ back to the original
______________________________
- disturbing the __________________________ can cause the
extra _________________ to “_____________________________” of
solution (______________________________ out)
Solubility Curves
Points that fall ____________ the line - ________________________
Points that are ___________ the line - ________________________
Points that are ____________ the line - ________________________
Examples:
1) What type of solution is formed from 40 g of KNO3 at 50oC?
2) At what temperature would 30 g of KClO3 form a saturated solution?
3) How many grams of Pb(NO3)2 can dissolve in 200 g of water at 40oC?
4) If a saturated solution of KCl is cooled fro 80oC to 30oC, how many grams
of KCl will precipitate out?
Factors Affecting
Solubility
Solids in Liquids
- Temperature: most __________________ will be ____________
soluble at ______________________ temperatures
Gases in Liquids
- Temperature: Gases become ________________ soluble at
_______________________ temperatures because the gas
particles have _________________ energy to ___________________
the top of the liquid and ___________________________
- Pressure: Gases become ________________ soluble as the
pressure above it ________________________
Essential Question __________________________________________________________________________
_________________________________________________________________________________________________
Concentration
Solutions can be described:
1) Qualitatively:
- Concentrated - there is ______________________ of solute
- Dilute – there is a _____________________________ of solute
2) Quantitatively:
Equation:
Molarity (M) =
It’s shown with the _____________________ of a solution.
Ex. 1.5 M NaCl (aq) is described as “1.5 molar”
Examples
1) What is the molarity when 2.0 moles of glucose is
dissolved in 5.0 L of solution?
2) How many grams of Na2SO4 would be required to
make 1.5 L of 0.24 M solution?
Dilutions
Can start with a solution of ______________ concentration
and add __________________ to ____________________ the
concentration
Equation
Example
What volume of 2.00 M CaCl2 would be needed to make
0.50 L of 0.300 M CaCl2?