Chemistry
Unit 9– Chapter 15 – Solutions (standard 6)
Name __________________________________ P.__ Date__________
Turn in stamp sheet on the day of the test for a chance at full credit. Late stamp sheets will be ½ credit.
GET ANY INCOMPLETE WORK COMPLETED!!! Late work = 2pts if complete if done by day of test!
ASSIGNMENT
DATE TO BE
POINTS EARNED
COMPLETED
1) Bonds Review
2) Solutions Vocabulary with sketches
3) Crossword on Solutions Vocab
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4) PPT notes - Solvation
5) Coffee – PPT note review
6) PPT notes – Factors that affect
solvation
7) IF Solubility curve worksheet
8) More Solubility Practice
9) Wordsearch – vocab refresher and
Mole calculation review (2 pages)
10) PPT notes – concentration calculations
11) Percent solution calculations
12) Parts per Million (ppm) worksheet
13) To Drink or Not to Drink analysis
worksheet
14) PPT notes - Molarity
15) IF Molarity calculations
16) 2 pages – Concentration Calculations
17) Standards Review
18) Fill in Review
#1
Bonds Review
Name:_____________________________Date: _____________________ Period:___
Directions: This assignment should help you review your standard 2.0 bonds material so that we can apply it
to our study of solutions. If you don’t remember any of the concepts, I expect that you will look them up in
your notes (the beginning of semester 2) or in your book (under ionic, covalent, or metallic bonds.)
1. Potassium (K) and chlorine (Cl) form a(n):
a. Covalent bond. b. Hydrogen bond.
c. Ionic bond.
d. Metallic bond.
Why? _________________________________________________________________________________________
2. When atoms combine to form a molecule by sharing electrons, what types of bonds are formed?
_______________________________________Why? __________________________________________________
3. A metallic bond is formed between:
a. A metal atom and a hydrogen atom.
b. A metal atom and a nonmetallic atom.
c. A metal atom and a noble gas.
d. Two metal atoms.
4. A scientist discovers a new compound. After chemical testing, the compound is found to have a high melting
point and high boiling point. What type of bond holds the compound together?
_____________________________________Why? ____________________________________________________
5. Which of the following is not a property of metals?
a. Malleability
b. ductility
c. brittle
d. shiny
6. Which do not form covalent bonds?
a. Diatomic molecules
b. Large biological molecules
7. The bonds found in C2H4 are:
a. Non-Polar Covalent
c. Molecules containing carbon
b. Ionic
c. Metallic
8. What type of bond holds each of the following together?
a. AlBr3
b. CO2
c. KCl
d. Salts
d. Polar Covalent
d. NaF
9. Some of the molecules found in the human body are NH2CH2COOH (glycine), and C6H12O6 (glucose). The bonds
they form are:
a. Nuclear
b. metallic
c. ionic
d. covalent
Why? _________________________________________________________________________________________
10. At room temperature, which substance has the weakest intermolecular forces?
a. Oxygen gas
b. Salt
c. Steel
d. Uranium
Why? _________________________________________________________________________________________
11. This state of matter occurs when there is a small amount of intermolecular attraction between molecules.
a. Solid
b. Liquid
c. Gas
d. Plasma
12. Which of the following shows increasing intermolecular forces (as read from the left to the right)?
a. Solid, gas, liquid
b. Solid, liquid, gas
c. Gas, liquid, solid
d. Liquid, gas, solid
13. A molecule of F2 gas is held together by:
a. Polar covalent bond
b. non-polar covalent bond
c. ionic bond
d. metallic bond
14. Which of the following will have the strongest intermolecular forces?
a. HF
b. CH4
c. NaCl
d. Cu
Why? _________________________________________________________________________________________
15. Electrons involved in a polar covalent bond are:
a. Transferred
b. shared equally
c. shared unequally
d. overlapped
16. Which statement best explains why CH4 is a non-polar molecule?
a. CH4 has a symmetrical charge distribution
b. C and H are non-metals
c. C and H have the same electronegativity
d. CH4 has four bonds.
17. Compared to intramolecular bonds, the strength of intermolecular forces are:____________________________
18. Draw the lewis dot structures for:
a. Si
b. Al
c. As
d. Ga
UNIT 9 – SOLUTIONS VOCABULARY
TERM
1. aqueous
2. colligative
3. concentrated
4. dilute
5. dissociation
6. electrolyte
7. equilibrium
8. heterogeneous
mixture
DEFINITION
SENTENCE
#2
PICTURE
9. homogenous
mixture
10. miscible
11. saturated
12. solubility
13. solute
14. solution
15. solvent
16. unsaturated
#3
Directions: Complete the crossword.
Name:______________________________
Date: _____________ Period:___________
#4
Solvation Notes
date:__________
What is a solution ?
 A solution is a mixture of 2 things, the ____________ and the _____________________.
 Another word for a solution is a ____________________.. A homogenous mixture is when 2 or
more things are mixed, but you only see one thing.
 A ____________________. is what dissolves or disappears, like salt or sugar.
 A ____________________. is what does the dissolving. It is what you see when you look at a solution.
Water is called the ____________________..
 You will always have ____________________.than solvent.
 Solvation is the scientific way of saying “____________________.”
Examples:
 Salt water
 70% ethanol solution.
 What is the solute?___________
 Solute _______________
 What is the solvent?___________
 Solvent________________
 Why?
Studying Solvation
 We want to____________________.what solutes will dissolve in which
solvents.
 In order to do this, we need to know what ____________________.the
solute and solvent are.
 The type of molecule and the IMFs that form will help us to determine if
solvation will occur.
 ____________________.will hang out with each other to form
a solution
 Molecules that are not alike will____________________.from
each other.
Bond Review
 How can you tell if a molecule is ionic, polar covalent, non-polar
covalent, or metallic?
 Ionic:
 Electronegativity difference of ____________________.
 1st element in groups 1-3, metals, 2nd element is in groups
5-7 non-metals
 ____________________. IMF
 Metallic: ____________________.combining electrons
 Covalent:
 Polar has ____________________.of e- on central element
(usually grps 5 or 6) or
 Polar will have 2 ____________________.bonded to central
element (usually groups 3 or 4)
What type of bonds hold the following compounds together?
 KCl ____________________.
 CO2 ____________________.
 H2O ____________________.
 Sugar ____________________.
 CaCO3 ____________________.
 Benzene ____________________.
Water
 Water is a ____________________. molecule. Why? Because oxygen has
H
____________________.
 This means the oxygen ____________________.charged and both
hydrogens are positively charged. Why? Because oxygen
____________________.____________________.
 What type of IMFs will water have?
 Polar molecules can have dipole-dipole or hydrogen bonds. Water has both
O, so molecules are held together by
__________________________________________________.
H
O
H&
Ionic Solubility Rules
We can predict if a solute will dissolve in a solvent by using looking at the bonds of each molecule.
“Like Dissolves Like”
 Ionic or Polar solutes will dissolve in ____________________.solvents
 Alcohols (ending in –ol or OH) will dissolve anything BUT ____________________..
 Ethanol, methanol, isopopanol are alcohols and will dissolve anything except polar solids like
sugar.
 Water is considered a ____________________.because it can dissolve both ionic and polar covalent
compounds
Ionic Compounds in Water
 In an ____________________., water is the solvent.
HCl (aq), NaCl(aq), CuSO4 (aq)
 Ionic solutes will ____________________. into its ions when ____________________. in water. Why?
 Because the charged parts of ionic bonds are ____________________.to the charged parts of
water.
 NaCl (in water)  ________________________________________.
 K2SO4 (in water ) ________________________________________.
Ionic Solvation: NaCl and Water
1. Salt solute is added to water.
2. Salt ________________________________________.until it bumps into or “hits on” the water molecules.
The Na+ part of the salt is very ____________________. to the bad boy Oxygen and his negative charge.
The Cl- part of the salt is very ____________________. to the good little girl Hydrogen and her positive
charge
3. Salt ________________________________________.up into Na+ and Cl-.
4. Each ion is completely ____________________. by water molecules “groupies!”.
_______________________________________________________________________________..
Polar Covalent Solvation: Sugar and Water
1. Sugar solute is added to water.
2. Sugar will _________________ move around until it bumps into the water molecules.
3. The partially charge part of the sugar molecule is very ____________________ to the oppositely charged
part of the water molecules.
4. The covalent solute (_________________) _________________________________.
5. Instead, the sugar is a _________________ by staying bonded and forming a ________________
relationship with the water.
6. When the sugar is completely _____________________ by solute “groupies” (aka water) we say it has been
________________________________.
Solvation PowerPoint Notes REVIEW!
1. If lithium chloride (LiCl) is dissolved in water, water is the: (std 6a)
a. solute
b. solvent
c. solution
#5
Why?____________________________________________________________
2. A teaspoon of dry coffee crystals dissolves when mixed in a cup of hot water. When the crystals are placed in a
cup of hot water a coffee solution is created. The dry coffee crystals are classified as: (std 6a)
a. solute
b. solvent
c. reactant
d. product
Why?____________________________________________________________
3. Which of the following would be expected to dissolve easily in water (think solubility)? (std 6b)
a. CH4
b. H2
c. SiF4
d. CCl4
e. NaNO3
Why?____________________________________________________________
4. If the attractive forces among two or more solid particles are not as strong as the attractive forces between the
solid particles and water molecules, the solid will: (std 6a)
a. probably form a new precipitate as its’ crystal lattice is broken and reformed
b. be unaffected because attractive forces within the crystal lattice are too strong to dissociate
c. begin the process of melting to form a liquid
d. dissolve as particles are pulled away from the crystal lattice by the water molecules
Why?____________________________________________________________
5. Oil and water will ________________. (std 6b)
a. mix because both are polar molecules
b. not mix because water is polar and oil is nonpolar
c. mix because both are nonpolar molecules.
d. not mix because oil is polar and water is nonpolar
6. When CaCl2 dissolves in water, what part of the water molecule will the Calcium ion be attracted to? (std 6b)
a. the oxygen end, which is negatively charged
c. the oxygen end, which is positively charged
b. the hydrogen end, which is positively charged d. the hydrogen end which is the negatively charged
Why?____________________________________________________________
7. The general rule which determines whether substances will mix is: (std 6b)
a. Like polarities dissolves like
c. Opposites attract
b. Solutions are homogeneous mixtures
d. Solvents and solutes don’t mix
8. KCl is added to water. The KCl will randomly move around until it collides with a water molecule. Different
parts of the KCl molecule are attracted to water and will eventually _____________. (std 6b)
a. saturate
b. dissociate
c. dilute
d. associate
Why?____________________________________________________________
9. Why does increasing the temperature increase the solubility of solids? (std 6b)
a. because hot molecules are more attractive
c. faster molecules collide more often
b. water surrounds hot molecules more quickly
d. hot molecules dissociate more quickly
10. How does the dissolving of sugar differ from the dissolving of salt in water?
Factors that Affect Solvation – PPT notes
We can speed up the process (of solvation) in a couple of ways:
 ___________ or stir the mixture
 Increase the ____________ (solids or liquids only)
 Increase the ________________ of solute
 Increase the ______________ (gases only)
#6
Why does each of the above work? Because it will increase the ____________________________!
Solubility Curves
• Solubility depends on the molecule and the ___________
• Graph allows us to _____________ the solubility under different temps
• Which one is the only molecule where solubility decreases as you increase
temp? _________________Why? _________________________
Solubility Curves Questions
• What is the solubility of KCl at 70°C? _________
• How many grams of KClO3 will dissolve in 100 grams of water at 40°C ?
_____________
• How many grams of KClO3 will dissolve in 50 grams of water? ________
• Precipitates
• If a saturated solution cools down, it can no longer keep as much ___________ dissolved. So as it cools some of
the solute will “_______________________” and you will see a solid settling out. This solid which has “fallen out
of solution” is called a __________________.
• Precipitate is abbreviated – ___________.
• PPT example 1 –
80 g of KNO3 is dissolved in 100g of water at 50°C. Is
this saturated, unsaturated or supersaturated?
• PPT example 2 –
100 g of KNO3 is dissolved in 100g of water at 50°C. Is
this saturated, unsaturated or supersaturated?
PPT example 3 –
130 g of KNO3 is dissolved in 100g of water at 70°C.
The solution is cooled down to 40°C. How much
KNO3 is going to fall out as a precipitate?
#7
More Solubility and Solubility Curve Questions
#4
1) How much KNO3 can dissolve in 100g of water at 70oC?
2) How KNO3can dissolve in 50g of water at 70oC?
3) Although Ce2(SO4)3 is an ionic solid, a student may think that it is a gas based on its
solubility. Explain why they may think this.
4) Which is more soluble in water at 50 oC, KNO3 or NaNO3?
5) 40 g of KClO3 is dissolved in 100g of water at 80oC, how much precipitate will form if
the solution is cooled to 50 oC?
6) What is a precipitate?
Decide if the solution is U (unsaturated), S (saturated), or SS (supersaturated). (put a point on
the graph, if it is on the line =S, above = SS, and below = U)
7) _____ 50 g of KCl in 100g of water at 80 oC.
8) _____ 60 g of NH3 in 100g of water at 10 oC.
9) _____ 150 g of KI in 100g of water at 20 oC.
10) _____ 145 g of KI in 100g of water at 20 oC.
11) _____ 140 g of KI in 100g of water at 20 oC.
12) _____ 150 g of KI in 200g of water at 20 oC.
13) Explain why we say that “sugar” is cheating when it dissolves into water? Use pictures if necessary
14) Why do we say that the ions of salt get surrounded by water “groupies”?
15) Give 3 factors that can increase the rate of solvation and explain why.
Huh? A Refresher for the Solutions Unit
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#9
___________________________1 ) A solution with water as the solvent.
___________________________2 ) A property determined by the number of dissolved particles in a solution.
___________________________3 ) When a solution has a lot of solvent dissolved in the solution.
___________________________4 )
___________________________5 )
___________________________6 )
___________________________7 )
___________________________8 )
to be in _______
___________________________9 )
___________________________10 )
___________________________11 )
___________________________12 )
___________________________13 )
___________________________14 )
___________________________15 )
___________________________16 )
slightly negative end.
___________________________17 )
___________________________18 )
___________________________19 )
___________________________20 )
___________________________21 )
___________________________22 )
A_______compound is formed of only nonmetal atoms.
A _______solution has very few solute particles dissolved in the solvent.
_______is the separation of an ionic compound into its ions.
A substance that will conduct electricity when dissolved in water.
When the rate of dissolving = the rate of crystallization the solution is said
_______become less soluble as the temperature of the solvent increases.
In a _______mixture the particles are not uniformly mixed and are visible.
_______ mixture is another name for a solution.
A_______compound is formed of metal atoms with nonmetal atoms.
_______ dissolves like.
Two liquids that can dissolve into each other are said to be _______
A combination of 2 or more substances.
Water is considered to be _______ since it has a slightly positive end and a
A solution that cannot dissolve any more solute is said to be _______.
_______ become more soluble in a solvent as temperature increases.
How well a solute dissolves.
The substance that is dissolved by a solvent.
The substance that dissolves a solute.
A solution that still can dissolve more solute is said to be _______.
Review of Molecular Weight and Mole Calculations
#9
1. What is the molecular weight of NH4Cl? Use your periodic table to look up the atomic
mass of each element – round to a whole number.
(atomic mass of N) + 4 (atomic mass of H) + (atomic mass of Cl) = molecular weight (g)
2. How many moles are in 100 g of NH4Cl? Use a T-chart.
100g of NH4Cl 1 mole of NH4Cl
g of NH4Cl
=
Fill in molecular
weight from #1
above
3. What is the molecular weight of Mg(OH)2?
4. How many moles are in 25 g of Mg(OH) 2? Use T-chart
#10
Concentration Calculations: % by Mass and % by Volume – PPT NOTES
% Calculations
 You can use __________________ to describe how much __________________ solute has dissolved in a liquid or __________________
solvent. All of your numbers need to be in __________________of mass (g, kg, mg etc.)
 You can use % by __________________ to describe how much __________________ solute is dissolved in a__________________solvent.
All of your numbers need to be in the __________________of volume (L, mL etc.)
% Vol 
mL solute
x100
Total mL solute  solvent
 Remember that the denominator has the total amount of solution, volume solvent + volume of solute!
 What is the concentration of 75 mL KBr in 2500 mL of water?
% Mass 
g solute
x100
Total g solute  solvent
 Be careful!! The denominator must have the __________________of the solution… g solute + g solvent!
 Ex: What is the concentration of a solution that has 5 g solute dissolved in 100 g solvent?
 What is the concentration of 20 g KBr in 600 g of water?
 How much water is needed to make a 15% solution with 5g of solute?
Name__________________________________Date: _________Period_________
#11
Percent Solutions
% by volume =
volume of solute
total volume of solution
%by mass= mass of solute(g)
Mass of solution (g)
1. What is the concentration in mass percent of the following solutions?
a. 20g of KCl in 600 g of water.
b. 32g of NaNO3 in 2000 g of water.
c. 75 grams of K2SO4 in 1500g of water
2. What is the percent by volume of methanol if 75 mL of methanol is added to 400 ml of water?
3. What is the percent by volume of hydrogen peroxide if 25ml of hydrogen peroxide is diluted to a final total volume of
150ml?
4. How much water will you need to mix with 5g of a compound to produce a 15% solution?
Parts Per Million
#12
Sometimes when concentrations are really small, we use parts per million to represent the
concentration instead of percent by mass or molarity.
Parts per million (ppm) =
grams solute X (1 x 106)
grams solution
Example - a chemical analysis shows that there are 2.2 grams of lead in exactly 500 grams of
water, what is the concentration of lead in ppm?
ppm = 2.2 grams X (1 x 106)
500 grams
= 4400 ppm
Complete the following problems.
1. A sample of 300.0g of drinking water is found to contain 38g of Pb. What is this concentration in ppm?
2. A solution of lead sulfate contains 0.425g of lead sulfate in 100.0g of water. What is this concentration in
ppm?
3. A 900.0g sample of sea water is found to contain 0.0067 g of Zn. Express this concentration in ppm.
4. A 365.0g sample of water contains 23g of Au. How much gold is present in the sample in ppm?
5. A 650.0g hard water sample contains 0.101g of Ca. What is the concentration in ppm?
1 More Thing… More Difficult % Problems
Sometimes, the problems will assume that you know the DENSITY of water in order to calculate % mass.
Density of water = 1g / 1 mL. You can use the density as a CONVERSION FACTOR
6. How much will 600 mL of water weigh?
7. What is the % concentration by mass of 15 g HBr dissolved in 600 mL of water?
Water Contaminants Reference Chart - EPA
Contaminant
Max
levels in
ppm
Potential Health Effects from
Long-Term Exposure Above the
MCL (unless specified as shortterm)
Increase in blood cholesterol;
decrease in blood sugar
Skin damage or problems with
circulatory systems, and may have
increased risk of getting cancer
Kidney damage
Antimony
0.006
Arsenic
0
Cadmium
0.005
Copper
1.3
Cyanide (as
free cyanide)
0.2
Fluoride
4.0
Bone disease (pain and tenderness
of the bones); Children may get
mottled teeth
Lead
zero
Infants and children: Delays in
physical or mental development;
children could show slight deficits
in attention span and learning
abilities
Mercury
(inorganic)
0.002
Selenium
0.05
Thallium
0.0005
People with Wilson's Disease
should consult their personal doctor
if the amount of copper in their
water exceeds the action level
Nerve damage or thyroid problems
Adults: Kidney problems; high
blood pressure
Kidney damage
Sources of Contaminant in Drinking
Water
Discharge from petroleum refineries; fire
retardants; ceramics; electronics; solder
Erosion of natural deposits; runoff from
orchards, runoff from glass &
electronicsproduction wastes
Corrosion of galvanized pipes; erosion of
natural deposits; discharge from metal
refineries; runoff from waste batteries
and paints
Corrosion of household plumbing
systems; erosion of natural deposits
Discharge from steel/metal factories;
discharge from plastic and fertilizer
factories
Water additive which promotes strong
teeth; erosion of natural deposits;
discharge from fertilizer and aluminum
factories
Corrosion of household plumbing
systems; erosion of natural deposits
Erosion of natural deposits; discharge
from refineries and factories; runoff from
landfills and croplands
Hair or fingernail loss; numbness in Discharge from petroleum refineries;
fingers or toes; circulatory problems erosion of natural deposits; discharge
from mines
Hair loss; changes in blood; kidney, Leaching from ore-processing sites;
intestine, or liver problems
discharge from electronics, glass, and
drug factories
#13
Real Life
Connection!
In the U.S. we are very lucky that most people of access to potable (drinkable) water. Safe water is not available
to many people in the world. In fact, every 20 seconds a child in the world dies due to
contaminated water. Not only are we lucky, many of us are even water snobs, preferring to
drink bottled water. (By the way, we didn’t drink bottled water until the 1980’s, ask your
parents or grandparents about that)
Not only do we have easy access to water, we even have a government agency, the
Environmental Protection Agency (EPA) that sets guidelines for the water that is delivered to
our homes (water coming into your sink). This agency has set up standards about the
allowable levels of contaminants in our water.
The attached chart indicates the levels for some of the many contaminants that are regulated. Use this chart to
help you decided the answers to some of the following questions.
1) Name a country where the people probably have trouble getting safe water to drink.
2) What does potable mean?
3) What does contaminant mean?
For the following – identify the contaminant that is linked to health effect listed and give 2 of its sources (how does it get
into our water)
4) Hair loss and liver problems
5) Fingernail loss and numbness in toes
6) Bone disease
7) Nerve or thyroid damage
Use the chart to help answers these questions
8) Which two contaminants have no safe levels in water and for each, describe the potential health effects if you were to
consume these chemicals.
9) Lydia Rogers has lost her hair and is suffering from liver and kidney problems. She thinks her drinking water has been
contaminated by thallium from the Corning glass company in the next city. She has hired Gloria Allred to represent her
in her lawsuit.
The EPA has tested her house’s water and found that in the 2000 mL sample there was 0.000008 mL of thallium. Could
her water be causing the problems? Explain your response and show your calculations of ppm.
10) Why do you think the allowable amount of Fluoride is so much higher than the other chemicals?
11) In a 5000 mL sample of water, what is the maximum volume of Fluoride allowed?
12) A 2000 mL water sample was tested and found to contain 0.0009 mL of benzene.
a) Calculate the % by volume of benzene –
b) Calculate the ppm for benzene –
c) Why do you think the EPA would prefer to use the ppm calculation instead of the % by volume?
13) So when should you use ppm for concentration instead of % by volume?
Sj12
#14
Concentration Calculations: Molarity PPT
Calculation Review
 The molecular weight of a molecule is calculated by _______________________ the atomic masses for
each atom in the molecule.
 Ex: AlCl3
 Ex2: Ca(OH)2
 We use moles to describe _______________________of a molecule we have.
 To calculate # moles, you need to do a t-chart and use the _______________________.
 Ex: How many moles are in 140 g of Cl2
 Ex: How many grams are in 0.5 moles of NaCl?
How do we know how much stuff has dissolved?
 We can’t see the solute that has dissolved, but we can _______________________ how much has
dissolved.
 There are _______________________ ways to calculate how much solute has dissolved.
 Molarity
 % by mass
 % by volume
 Parts per million (ppm)
Which one you should use depends on the _______________________ of solute, the
_______________________ of the solute, and the phase of the solvent.
Molarity
Molarity (M)  moles solute
L solvent
 Use molarity when you have a _______________________ solute and a _______________________
solvent
 Larger molarity values means a more _______________________ solution
 Ex: What is the molarity of a solution that has 2 moles of KOH in 4 L of water?
 What is the molarity of a solution that has 37.5 g of Ca(OH)2 in 0.25 L of water?
 How many grams of NaCl must be used to make a 2M solution with 3 L of water?
Molarity Calculations Handy Hints:
1) Start by calculating Molar Mass of solute unless given # of moles of
solute already.
2) Write down Molarity formula and fill in the numbers your given.
3) If your only missing one number in molarity formula, solve to
calculate the missing number OR if missing 2 numbers, you will need to use a
T-chart to figure out the moles of solute and then plug the # of moles back
into Molarity formula.
You will be given the Molarity formula on the test.
#15
#18
Solutions Test Fill-in Review
Fill in answers
% volume
1 000 000
100
5M
Areas
Collisions
Concentration
Differences
Dissolving
Gases
Increased
Into
Ionic
Less
Like
M
Masses
Molar mass
Moles
Nonpolar
Oil
Parts per million
Periodic
Polarity
Positive
Rip
Rise up
Saturated
Settle
Solubility
Solution
Solution
Solve
Solvent
Surface area
Symmetry
T-charts
Water
1) A ______________is made of a solvent and a solute.
There is more of the _____________and it is what
does the dissolving, hence the word “_________” in
both solvent and dissolve.
2) Basically what happens during solvation, or
__________, is that the molecules of solvent attack and
____ apart the solute molecules. The rate of solvation is
____________by stirring or heating which will increase
the number of ____________between solvent and
solute particles.
3) Solvation is also increased by increasing the
____________________of the solute, in other words,
breaking the solute into smaller pieces. This increases
solvation because the solvent molecules now have more
___________to attack on the solute.
4) But, __________ are less soluble in hot liquids than
cold liquids. This is because as a gas is heated, it expands
and will ____________into the atmosphere.
5) A ____________curve graph shows how increasing
water temperature will affect how much solute can
dissolve.
6) Whether a solute will dissolve in a solvent is
determined by________________. A polar or ionic
molecule has a ___________end and a negative end. A
____________molecule has no charges. Like
dissolve________, meaning polar dissolves polar or
__________and nonpolar dissolves nonpolar.
7) ___________is a very common polar molecule. All ionic compounds are
polar. A molecule that lacks _____________is often polar. __________ is a
very common nonpolar substance, so water and oil don’t mix due to the
______________in polarity.
8) __________________is an indication about how much solute is dissolved
L
in a solvent. Most solvents can only dissolve up to a certain amount of solutes.
Once a solvent dissolves as much as it can, we say it is _________________.
Extra solute will ____________on the bottom of the container.
9) Molarity, ppm, % mass, and ______________are all ways of describing
concentration. PPM, or_________________, is used when the amount of
solute is a lot _________than the amount of solvent. The calculations for
ppm, % mass, and % volume all involved dividing the amount of solute by the
total amount of ______________and then multiplying by _________(for %
mass and volume) or by ______________(for ppm).
10) Molarity calculations involve dividing the ____________of solute by
liters of solution. The unit for molarity is _____. Often molarity calculations
involve the use of ___________to convert grams of solute _______moles or
vice versa. To use the T-charts, the _________________ of the solute is
also calculated. The molar mass is found by using the _____________from
L
the ___________table for each element in the formula for the solute.
11) So a ________ HCl solution is much more concentrated than a 2 M HCl
solution.