Solutions
Student will learn:
solution terminology
3 ways to increase solubility
Solutions
Solution: one substance dissolved into another substance
3 types:
gas…..
liquid…
solid….
2 parts: solute = substance being dissolved……’smaller part’
solvent = substance doing the dissolving …’larger part’
Ex:
salt water
carbonated pepsi
Kool-aid
Heterogeneous = a visible mixture of 2 or more
Homogenous = one kind
lemonade
How to speed up dissolving?
l. Stir
2. Increase surface area….
grind large chunks into small grains
3. change temperature of solvent
a. increase temp…..solid in a liquid
b. Decrease temp…..gas in pepsi
Why are GASES ARE MORE SOLUBLE
IN COOLER SOLVENTS ??????
A solid dissolves faster in a liquid if
the temperature of the liquid is..
1. Increased
2. decreased
A gas dissolves faster in a liquid if
the temperature of the liquid is
1. Decreased
2. Increased
At which temperature will water in an
open vessel dissolve the greatest
quantity of oxygen?
1.
2.
3.
4.
5.
32OC
4OC
100OC
1OC
0OC
When a gas is being dissolved in a
liquid stirring _______ the
dissolving process.
1. Speeds up
2. Slows down
The student will :
if given a list of chemicals be able to determine
which chemicals will dissolve in which chemicals.
have conceptual understanding of electrolytes
identify electrolytes from a list of chemicals
Determining what will dissolve?
How do things dissolve?
Water is considered the universal solvent… water is a
polar molecule with + and – ends. The positive
end of a polar molecule will attract the negative end of another polar
molecular. Hence….
This is a review of dissolving in Chemical Bonding unit.
” like dissolves like”.
“polar dissolves polar”
“Nonpolar dissolves nonpolar”
How does one figure out if polar or non-polar ?
( all this is reviewed in chemical bonding unit)
1.
2.
3.
all Ionics are polar …. Metal + nonmetal
Draw Lewis structures
calculate electronegativity
1.7chart
Solubility ( polar vs non-polar)
“like dissolves like”
Polar molecules will dissolve polar molecules
Non-Polar molecules will dissolve Non-Polar molecules
Alcohols will normally dissolve both, both not ionic solids.
Solutes
1. NaCl
2. I2
3. Ca(OH)2
4. KCl
5. Br2
6. KNO3
7. CuSO4
8. CO2
9. FeO
Water
Carbon
tetrachloride
Alcohol
The student will :
if given a list of chemicals be able to determine
which chemicals will dissolve in which chemicals.
have conceptual understanding of electrolytes
identify electrolytes from a list of chemicals
Electrolyte: a solution that can conduct electricity
ex: ionic solutions, ionic compounds …
ionize into their separate ions when dissolved in water
“They separate into their + and - parts”
Non-electrolyte: a solution that cannot conduct electricity
ex: nonpolar solutions
non-metals and non-metals
do not have + or - ends
Demo: salt in water
Electrolytes
Electrolytes dissociate or ionize in water to produce ions.
Electrolytes are capable of conducting electrical current.
Electrolytes consist of ACIDS, BASES, IONIC COMPOUNDS
Chemical
1. NaCl
2. CCl4
3. C8H14
4. HCl
5. CuSO4
6. AgOH
7. KCl
8. H2O
9. H2SO4
10. FeO
Electrolyte
Non-Electrolyte
Which chemical would be a good prospect
as an electrolyte to add to an energy drink?
1.
2.
3.
4.
5.
6.
C2H5OH
N 2O 2
HCl
H2SO4
MgCl2
AuCl3
Student will be able to:
Read, interpret, analyze data
from a solubility chart
Solubility
how much will dissolve at a given temperature.
Unsaturated: can dissolve more solute
Saturated: dissolved all it can
Supersaturated: contains more solute
than a saturated
. ”unstable”
The student will be able to :
calculate the concentration of
solutions using the Molarity
formula.
calculate the needed grams for
creating specific solutions.
[concentration] of Solutions Expressed as …..Molarity
[M] = #moles of solute
liters of solution
1.
What is the molarity of a solution consisting of 45
grams of Sodium Chloride in 500mL of water?
2.
A chemist needs half a liter of a 2M solution of
ammonia. How do you prepare this solution?
3.
Calculate the concentration of a sodium hydroxide
solution containing 10.0 grams in 500mL.
4.
What is the molarity of a sulfuric acid solution
containing 196 grams per liter?
5. What mass in grams of solid calcium chloride is
dissolved in 2 liters of water to prepare a 1.2M
solution?
6. How many grams of Copper II Sulfate does a chemistr
need if he wants 2L of a 3M solution?
7. Calculate the molarity of a hydrochloric acid solution
that has a volume of 16o00mL and contains 382g of HCl.
8. You added 2 tablespoons of sugar (C6H12O6) to your
morning hot milk. Each tablespoon of sugar is
approximately 13 g. What is the sugar molarity of your
drink?
9. How many liters are required to make a 6M solution of
3moles of potassium hydroxide?
Student will be able to:
calculate the needed quantity of
concentrate to dilute to the desired
solution
Molarity by Dilution
M1V1 = M2V2
You use this when you already have a solution made and you just want to
dilute it to the concentration you want.
1. How much concentrated 12M Hydrochloric acid is
needed to prepare 300 mL of a 3.0 M solution?
2.
How much water should be added to 200mL of 18M Sulfuric
acid to have a l.5M solution?
3. How much of concentrated 15M Nitric acid should
be added to make a 1 liter solution of 2M.
4. How many milliliters of 12M HCl needs to be diluted
to 200mL to make a 3M solution?
5. What is the molarity of a solution made by diluting
30mL of 8.0M KBr to 500mL?
6. 100mL of commercially available 18M sulfuric acid is
diluted to 500mL. What is the new molarity or
concentration?
7. A chemist wants to concentrate a diulted solution of
sodium chloride. The chemist has one liter of 2M of the
salt solution. Ho much water does he need toevaporate
to achieve a 5.5M concentration?
8. How do you prepare 250-mL of .5M silver nitrate from a
concentrated solution of 3M silver nitrate.
9. How much concentrated 8M Chlorine Bleach(NaOCl)
needs to be diluted to make 500mL of 1M Bleach?
Student will be able to:
calculate the needed quantity of concentrate
to dilute to the desired solution