Solutions A SOLUTION is a mixture Most water is a alloy that ...alkisites.vansd.org/dgray/Assignments/Solutions summary...Non-pure gold (less than 24K) is a solution of silver and

Name: _____________________

Period: _____________________

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Unit 5: 1

Solutions

A SOLUTION is a mixture

that is homogeneous at the

molecular level.

A solution is a mixture that is so

well mixed that is the same

throughout, even down to the

molecules. Yet these molecules

can still be separated physically.

The solvent is what

dissolves the solute.

Saturated—When a solution cannot

dissolve more solute (it’s full).

Unsaturated—When a solution can

hold more solute (not full yet).

Supersaturated— When a solution has

more solute than it can hold (over full).

The solute will eventually fall out of a

supersaturated solution (settle out).

NON-Solution Mixtures

Colloids—a mixture that has

larger particles, like milk, may-

onnaise, egg whites. The parti-

cles come in clusters, not single

molecules (like in solutions)

and they don’t settle (like in suspensions).

Suspensions—a temporary mixture in

which the particles eventually settle.

Suspensions can be easily filtered.

Silt in water (dirt kicked up in water)

is a common suspension.

Some colloids exhibit the

Tyndall effect, which is

the scattering of light as

it passes thru. Light

scattering in fog is the

Tyndall effect.

Solutions No

Colloids Yes (some)

Suspensions Yes

No

No

Yes

Molecular (smallest)

Slightly larger (in clusters)

Larger particles (often visible)

No

No

Yes

Mixture Particle size Scatters Light? Settles? Separated by filtering?

Soluble—

something

that can be

dissolved.

Insoluble—

something

that cannot be

dissolved.

Oil is

insoluble in water.

Sugar is

soluble in water.

Soluble vs. Insoluble

18 K

Non-pure gold

(less than 24K) is a

solution of silver and gold.

A alloy is a solution of two

metals melted together. When something goes

into solution (mixes in)

we say it dissolves.

Salt dissolves into water to

make salt water—a solution.

Common solutions:

salt water (salt dissolved

in water); syrup (sugar

dissolved in water).

Most water is a

solution because

there are dissolved

minerals in it.

Companies dis-

solve particular

minerals in

bottled water to

add flavor because

pure water has no taste at all.

Solvent vs. Solute

Water is the

solvent because

it is dissolving

the salt.

Salt is

the solute

because it is

what is being

dissolved.

Salt Water

Concentration How much solute is dissolved in the solution we call the concentration.

A solution with more solute is more concentrated.

Example: 100 mL of water can

hold 40 g of NaCl at 60º C.

40 g of NaCl is saturated (full).

30 g of NaCl is unsaturated

(it can still hold 10 g more).

50 g of NaCl is supersaturated

(it has 10 g too much).

If a solution

is too

concentrated

you can dilute

it by adding

more solvent.

Adding water to salt water dilutes

it—making it less concentrated.

Suspensions and colloids are mixtures that seem like solutions, but are not.

The particles are bigger and are not actually dissolved in the liquid.

Name: _____________________

Period: _____________________


Unit 5: 1

Soluble or insoluble in water:

Cooking oil ______________

Sugar ___________________

Soap____________________

Dirt ____________________

Salt ____________________

Ionic compounds _________

Solution (So), suspension (P), or colloid (C)?

It settles ___________________________

Doesn’t settle or scatter light ___________

Scatters light, but doesn’t settle _________

Can be filtered ______________________

Homogeneous at molecular level ________

Particles sometimes visible ____________

Circle the solute and underline the solvent.

Salt water

Sugar water

A solution of 20% HCl and 80% water.

Chocolate milk

Rubbing alcohol: 60% alcohol; 40% water.

1. Solution

2. Alloy

3. Dissolve

4. Suspension

5. Colloid

6. Insoluble

7. Homogenous

A. When a substance cannot be dissolved into a solution.

B. A mixture that is the same throughout.

C. A mixture of two metals.

D. A mixture that is homogeneous at the molecular level.

E. When something seems to disappears into a solution.

F. A mixture that scatters light and the particles do not settle.

G. A temporary mixture; the particles will eventually settle.

1. Tyndall Effect

2. Supersaturated

3. Saturated

4. Solute

5. Unsaturated

6. Solvent

7. Dilute

A. To lessen the concentration of a solution (add solvent).

B. When a solution can hold more solute.

C. When a solution can’t hold more solute.

D. When a solution has more solute than it can hold.

E. The part of the solution that dissolved.

F. The scattering of light in a colloid.

G. What is doing the dissolving.

Circle all of the Solutions 50 mL of a solvent can hold 80 g of a solute, are the

following saturated, unsaturated, or supersaturated?

_____ 35 g.

_____ 80 g

_____ 82 g

_____ 100 g

_____ 75 g

_____ 81 g

Salt water

Sugar water

Drinking water

Orange juice

Pure gold

Iron

Steel

Oil and water

Soap and water

Which one is more concentrated?

A 35% solution or a 46% solution?

A supersaturated solution or a saturated solution?

Thin syrup or thick syrup?

A saturated solution or an unsaturated solution?

A diluted solution or an undiluted solution?

B C A

___ The colloid.

___ The solution.

___ The suspension.

___ A mixture.

___A substance.

___Will settle.

___Can be separated

physically.

A salt solution is too concentrated. How would you dilute it?

What will eventually happen to a supersaturated solution?

What does it mean when a suspension settles?

before after If the two pictures show

what happens to a mixture

after a time, what kind of

mixture is it and why?

What happens if you add more solute to a saturated solution?

What happens if you add more solute to a supersaturated

solution?

What happens if you add more solute to an unsaturated solution.

A liquid is poured onto a piece of metal. Later on the metal

seems to have softened.

A) Which is the solvent?

B) What is happening to the metal?

Name: _____________________

Period: _____________________


Unit 5:

Name: _____________________

Period: _____________________


Unit 5: 2

Water—the (Nearly) Universal Solvent

Why does water dissolve so many solutes?

Because water is a polar molecule.

Polar molecules have positive and negative sides.

(Like magnets have north and south poles.)

H+

O-

H+

H+

O-

H+

H+

O-

H+

H+

O-

H+

A water “chain” is held together

by molecular cohesion. This

attraction between the negative

oxygens and the positive hydro-

gens is called a hydrogen bond.

These internal electromagnetic

forces (opposites attracting) are

responsible for water tension (why

bugs can walk on water) and

capillary action (how plants can

“suck up” water from their roots).

– 6 v.e.

8 shared O H

H 1 v.e.

2 shared

1 v.e.

2 shared

Positive side (Hydrogen

without its one electron

leaves a proton).

Negative side

(Oxygen with 2

extra electrons from

the Hydrogens).

+

The Covalent Water Molecule.

Ionic compound are made up

of positive and negative ions.

When placed in water, the

polarity of water pulls the ions

apart (called dissociation) and

the compounds dissolves.

Polar molecules will dissolve

in water. Nonpolar molecules

will not (like oil).

Salt (NaCl) dissolved in water.

Stirring —speeds up how fast

the solvent touches the solute and

moves solute into unsaturated

regions of the solvent.

Increasing Temperature —

speeds up how fast the solute dissolves

because increased temperature means

faster moving molecules AND more

room for more solute (see below).

Water is called the “nearly” universal solvent because it dissolves so many things.

Water will dissolve ionic and polar compounds, but NOT non-polar ones, like wax or oil.

The Oxygen atom

has more protons than

the Hydrogens and,

close to a full shell,

is more attractive to

the electrons, so the

electrons from the

Hydrogens spend more

time around the Oxygen.

Crushing (make particles smaller)

—Smaller particles really mean more

surface area for the solvent to touch

the solute (more sides available).

Powders dissolve faster than cubes.

When liquids heat up they expand (a bit). The extra space between

molecules affects solids differently than gases, since solids tend to sink

and gases tend to rise (and are compressible).

Cold liquid: closer molecules, so

more gas can be trapped inside.

Cold liquid: less solids can fit

between the closer molecules.

Warm liquid: more room between

molecules, so gases can escape.

Warm liquid: more solids can fit

between the spread out molecules.

Increasing Amount Dissolved

Changing Dissolving Rate

Temperature

Increasing pressure

forces more gas

into solution

(holding it in). This

is why colas fizz

when opened. The

CO2 is forced in

under pressure: release the pressure

(open it) and the gas escapes. Since

solids are not compressible, pressure

has no effect on solid solutes.

Increasing Pressure (gases only)

Na+

O- H

+

H+ Cl-

O-

H+

H+

O-

H+

H+

O-

H+

H+

O-

H+

H+

O-

H+

H+

O-

H+

H+

The negative Chlorines are attracted to

the Hydrogens; the positive Sodiums are

attracted to the negative Oxygens.

c

Solid

Gas

Liquid

(solvent)

Name: _____________________

Period: _____________________


Unit 5: 2

Polar or Non-polar?

1. Dissolve

2. Pressure

3. Crushing

4. Heating

5. Stirring

A. Causes more gaseous solvent to be forced into a liquid.

B. Increases solubility by moving the molecules around faster.

C. Increases solubility by allowing the solvent to touch more sides of the solute.

D. Expands the solvent a bit to allow more room for the solute.

E. When something seems to disappear inside a solvent.

1. Water tension

2. Dissociation

3. Hydrogen bonds

4. Polar Molecule

5. Capillary action

6. Cohesion

A. The breaking up of an ionic molecule by a polar solvent.

B. A molecule that has a positive and negative end.

C. The attractive force between two molecules of the same substance.

D. The attractive force caused by hydrogen protons to a more negative non-metal.

E. What allows plants to draw water up from their roots.

F. Caused by the cohesion of water molecules holding it together.

1. Solute

2. Solvent

3. Covalent

4. Ionic

5. Concentration

A. The part that dissolves into the solution.

B. The part that dissolves something.

C. Compounds made up of two non-metals.

D. Since they are made up of ions, they are polar molecules.

E. Tells you how much solvent is dissolved in the solution.

___ Cooking oil

___ Soluble in water

___ A compound with H’s

___ Sugar

___ Salt

___ Ionic Compounds

___ Dissolves in water

___ Insoluble in water

Give three ways to make sugar dissolve faster.

Draw a water molecule, being sure to label the ends as positive

and negative.

Do metals become positive or negative?

Would a metal be attracted to water’s hydrogens or oxygen?

Would a nonmetal be attracted to water’s hydrogens or oxygen?

To which side of a Water Molecule are these Attracted?

____ Magnesium

____ Chlorine

____ Calcium

___ Sulfur

___ Potassium

___ Helium

____ Iron

____ Bromine

____ Nitrogen

Which is the smallest particle size: rock salt, regular salt,

or finely powdered salt?

Which is the largest particle size: sugar cubes, granulated sugar

(regular table sugar), or powdered sugar?

Which one will dissolve the fastest?

Powdered sugar or granulated sugar?

In hot water or in cold water?

Stirred or not stirred?

Large particles or small particles?

OR

Which holds more solid solute: hot or cold liquids?

Which holds more gaseous solute: hot or cold solvents?

What property of gases allows them to be pressured into

solution?

Which is warmer: artic water or tropical water?

Which holds more oxygen: artic water or tropical water?

When power plants use cold streams for cooling, they can kill the

fish by heating up the water. Why do many fish die?

Why are water bugs able to “walk on water”?

How do plants get water from their roots up to their leaves?

Name: _____________________

Period: _____________________


Unit 5:

Name: _____________________

Period: _____________________


Unit 5: 3

Acids and Bases

pH—The Measure of Acids and Bases

7

Neutral Acids Bases Weak acids Strong bases Weak bases Strong acids

14 0 8 9 10 11 12 13 1 2 3 4 5 6

Lemon juice

Vinegar Distilled water

Baking soda

Bar soap

Ammonia Concentrated HCl

Concentrated NaOH

Neutralization (Titration)

Acids Bases

NaOH—

sodium hydroxide:

a very strong base.

In water it breaks up

(dissociates) making

OH– ions.

HCl—

Hydrochloric acid:

a very strong acid.

In water HCl breaks

up (dissociates)

making H+ ions.

O-

H

OH– ion O-

H Na+

Na+

In water

Cl-

H+ Cl-

H+

In water H+ ion

Many of our foods are acidic: citric (lemons; oranges); apples; tomato sauce. Acids taste sour and feel “squeaky” when you rub your fingers together.

Many of our cleaning products are basic (ammonia [Windex]; soap; bleach) because they neutralize acidic food. Bases taste bitter and feel slippery.

Strong acids and bases —ionize almost

completely in water, contributing many ions.

Strong acids and bases can burn your skin or eyes.

Weak acids and bases—ionize incompletely,

contributing just a few ions.

When acids and bases are mixed they neutralize each other.

Equal concentrations of acids and bases make neutral salt water.

HCl + NaOH → NaCl + H2O

Acid + Base → Salt Water

A typical neutralization reaction:

H+

O-

H+

H+ O-

H

→

H+ + OH− → → → → H2O

+

One of the products

of a titration

is always water!

Acids are compounds that add H+ ions

to a water solution.

Bases are compounds that add OH- ions

to a water solution.

Diluting Acids

Chemists call ANY ionic

compound a salt. NaCl is

a special salt: table salt.

Never add water to a concentrated acid!

Always add acids to water!

water

acid

When acid compounds are dissolved in water,

heat is produced (sometimes a lot of heat). Acids

are more dense than water, so if you add water to

a concentrated acid, water sits on top and can

flash boil (quickly boil).

The boiled water can

splash up burning you

with hot water and acid.

If the acid is added to

water it sinks thru the

water and is diluted

safely.

Name: _____________________

Period: _____________________


Unit 5: 3

1. Acid

2. Base

3. Neutral

4. Neutralize

5. Acid Rain

6. A Salt

7. Table salt

A. To mix acids and bases to cancel each other out and make salt water.

B. A compound that adds H+ ions to water.

C. Any ionic compound.

D. Equal number of H+ and OH– ions; water is an example.

E. A compound that adds OH– ions to water.

F. A compound of sodium and chlorine.

G. When pollution causes rain to be acidic (pH of less than 5.6).

1. pH

2. Salt Water

3. Strong Acid

4. Weak Base

5. Weak Acid

6. Titration

A. The measure of acids and bases.

B. A compound that adds a few OH– ions

to water.

C. To neutralize an acid with a base.

D. The product of a neutralization reaction

between an acid and a base.

E. A compound that adds a few H+ ions to

water.

F. A compound that adds a lot of H+ ions

to water.

pH and Acid Rain

Plants and animals need water close

to neutral (pH 7) to survive.

Due to pollution from combustion

reactions, rain today can be acidic.

Raid less than pH 5.6 we call acid

rain.

Acid rain can kills plants, cause

asthma and other physical problems.

Acid rain also eats away statues and historical

landmarks.

The Roman ruins, the pyramids of Egypt, and

other treasures of the world are being slowly

dissolved away by acid rain. More damage

has been done in the last century than in the

last 2,000 years.

Without stopping pollution (and acid rain)

these treasures may be lost forever.

___ Has fewer OH– ions

___ Has more H+ ions

___ Feels squeaky clean

___ Has fewer H+ ions

___ Tastes bitter

___Has more OH- ions

___pH of 0 to 7

___pH of 7 to 14

___Feels slippery

___Tastes sour

Solution A (pH 4); Solution B (pH 2)

Which one has more H+ ions?

Which one has less OH– ions?

Which one is more basic?

Which one is more acidic?

Solution A (pH 11); Solution B (pH 13)

Which one has more OH- ions?

Which one has less H+ ions?

Which one is more acidic?

Which one is more basic?

What is the product of every titration?

Finish these neutralization reactions: (balance the salt, too).

HBr + Mg(OH) →

HS + Li(OH) →

Should you add an acid or a base?

You need a pH of 6.2; you have a pH of 5.1.

You need a pH of 12; you have a pH of 13.4.



Acid or Base?

___ HCl

___ H2(SO4)

___ Mg(OH)2

__ H2(CO3)

__ NaOH

__ Ca(OH)2

__ H3PO4

__ LiOH

__ HNO3

Acid or Base?

How do you safely dilute a concentrated acid?

Antacids neutralize stomach acid. What is an antacid really?

Name: _____________________

Period: _____________________


Unit 5:

Name: _____________________

Period: _____________________


Unit 5:

Type Description Atomic Changes

Alpha Decay

Low energy particle. Helium nucleus:

2 protons; 2 neutrons;

stopped by paper or skin

Mass number: - 4 (2p + 2n)

Atomic number: - 2 (protons)

Beta Decay A Neutron splits into a proton and an

electron. Stopped by clothes or wood.

Mass number: no change

Atomic number: +1

Gamma Radiation

High energy radiation.

Stopped by lead or many feet of

concrete. Dangerous to living things.

No changes

Example

U-238 → Th-234 + α (Alpha particle)

C-14 → N-14 + β (Beta particle)

No changes

γ (Gamma ray)

If Fluorine 20 undergoes beta decay, what

will it become?

If Sulfur 34 undergoes alpha decay, what will

it become?

This is the decay series for Uranium-238. (Atomic numbers are on the bottom.)

On each arrow put either a “α” for alpha” decay or “β” for beta decay.

238

U→ 92

234

Th→ 90

234

Pa→ 91

234

U→ 92

230

Th→ 90

214

Po→ 84

210

Pb→ 82

210

Bi→ 83

210

Po→ 84

206

Pb 82

226

Ra→ 88

222

Rn→ 86

218

Po→ 84

214

Pb→ 82

214

Bi→ 83

Nuclear Power

Kinds of Radiation There are three kinds of radiation: alpha decay; beta decay; gamma rays.

Atoms can be changed The Greek philosopher Democritus believed there to be a smallest, indivisible particle:

atomos. In the early 20th century scientists learned that the atom is indeed divisible (can

be split) and even fusible (can be combined).

All Atoms are not Stable Neutrons add strong nuclear force without repelling the protons. That is why as atoms add

more protons, they have to add more neutrons (like glue) to keep the nucleus together. But

eventually the strong nuclear force is not strong enough.

neutron

+ +

proton

strong nuclear force

electro-magnetic repulsion

The strong nuclear force

is a short distance force. The electro-magnetic re-

pulsion of the protons is a

long distances force.

Eventually there are too

many protons and the re-

pulsion of the protons

wins. Over 83 protons and

the nucleus will undergo

radioactive decay.

Protons and

neutrons are

known as

nucleons

because they

are in the

nucleus.

Isotope Notation

C 14

6

Mass #: protons + neutrons

Atomic #: protons

S1

Name: _____________________

Period: _____________________


Unit 5:

Fission

Fission versus Fusion

Fusion

Large atoms are split apart. Uranium is

split into smaller atoms.

1 lb completely fissioned Uranium =

6,000 barrels of oil =

1,000 tons high-quality coal

Toxic radioactive waste

that takes billions of years

of decay to become safe.

Small atoms are fused together. Two

hydrogen atoms are fused into a helium atom.

1 km3 of sea water = more energy than all

known fossil fuels in the world.

Perfectly safe Helium.

We could make balloons.

There are two types of nuclear reactions.

Nuclear Process

Waste Products

Energy Produced

Half-life: the time it takes half of a radioactive substance to decay. Carbon-14 has a

half-life of 5,730 years. In 5,730 years 100 kg of carbon-14 would reduce to 50 kg.

Unfortunately, a radioactive substance never decays to zero; there’s always a half more.

The real winner: nuclear fusion. So why don’t we use it? Fusion occurs in the sun. It takes

millions of degrees to even start fusion. So far we can’t control it. But scientists are working on it.

As a future voter — demand money for fusion research!

Half-life

Carbon Dating Scientist use the known half-life of carbon-14 (5,730 years) to date plants, animals, and artifacts

less than 50,000 years old.. We know how much carbon-14 is in things when they die, so by

analyzing how much carbon-14 is in a sample today, scientists know when something died.

Chain Reactions In fission a neutron splits an nucleus. This produces another neutron (or more), which splits

another nucleus, making more neutrons, etc. A chain reaction is like toppling dominos.

1. Alpha Particle

2. Gamma Ray

3. Beta Particle

4. Radioactive

5. Uranium

A. The largest natural element. Fuel for fission reactors.

B. Can be stopped by wood; occurs when a neutron breaks into a proton and elec-tron.

C. An atom that emits energy or a particle is called this.

D. A helium nucleus (2 protons and 2 neutrons); low in energy.

E. Powerful radiation that can cause bio-logical damage; takes many feet of concrete to stop.

1. Chain Reaction

2. Fission

3. Fusion

4. Half-life

5. Carbon Dating

A. Combining smaller atoms into larger atoms. Harmless products; stars use this.

B. Splitting large atoms into smaller ones. Toxic by-products.

C. When one fission causes another and another, etc.

D. Using the known decay of an isotope to determine the age of objects.

E. The time necessary for 50% of a ra-dioactive sample to decay.

The sun uses fusion

and is the source of

all power on earth.

Nuclear power

plants use fission.

A simple example:

Half-life: 50 years

Starting mass: 400 kg

After 50 years:

(1st half-life)

200 kg left

After 100 years:

(2nd half-life)

100 kg left

After 150 years:

(3rd half-life)

50 kg left

After 200 years:

(4th half-life)

25 kg left

S1

Name: _____________________

Period: _____________________


Unit 5:

If Fluorine 20 undergoes beta decay, what

will it become?

If Sulfur 34 undergoes alpha decay, what will

it become?

This is the decay series for Uranium-238. (Atomic numbers are on the bottom.)

On each arrow put either a “α” for alpha” decay or “β” for beta decay.

238

U→ 92

234

Th→ 90

234

Pa→ 91

234

U→ 92

230

Th→ 90

214

Po→ 84

210

Pb→ 82

210

Bi→ 83

210

Po→ 84

206

Pb 82

226

Ra→ 88

222

Rn→ 86

218

Po→ 84

214

Pb→ 82

214

Bi→ 83

20 20

9 10

F20 = 9p and 11 e

F Nebeta

34 30

16 14

S34 = 16p and 18 e

S Sialpha

β α α

α α α

α

α

α

β

β β

β β

Chain Reactions In fission a neutron splits an nucleus. This produces another neutron (or more), which splits

another nucleus, making more neutrons, etc. A chain reaction is like toppling dominos.

1. Alpha Particle –D

2. Gamma Ray-E

3. Beta Particle-B

4. Radioactive-C

5. Uranium-A

A. The largest natural element. Fuel for fission reactors.

B. Can be stopped by wood; occurs when a neutron breaks into a proton and elec-tron.

C. An atom that emits energy or a particle is called this.

D. A helium nucleus (2 protons and 2 neutrons); low in energy.

E. Powerful radiation that can cause bio-logical damage; takes many feet of concrete to stop.

1. Chain Reaction-C

2. Fission-B

3. Fusion-A

4. Half-life-E

5. Carbon Dating-D

A. Combining smaller atoms into larger atoms. Harmless products; stars use this.

B. Splitting large atoms into smaller ones. Toxic by-products.

C. When one fission causes another and another, etc.

D. Using the known decay of an isotope to determine the age of objects.

E. The time necessary for 50% of a ra-dioactive sample to decay.

Name: _____________________

Period: _____________________


Unit 5:

Dissolving Lab

Purpose –

To demonstrate how various factors influence solubility including temperature, surface area (particle size), and agitation.

Preparation and Materials –

Three sources of water of varied temperature: ice water, room temperature, hot water (Hotplates or Bunsen burners). One large

Erlenmeyer flask will suffice for each.

Sugar cubes (large particle), granulated sugar (medium), powdered sugar (small) for three varied particle sizes.

Stirring sticks or spoons to agitate the water.

Timers to record the amount of time for the solute to completely dissolve.

One beaker per lab group.

NOTE: Powdered sugar contains corn starch, which will not dissolve, leaving the water cloudy. You may have to do an untimed

trial to learn to distinguish when the powdered sugar is dissolved and the only corn starch remains.

Data Tables

How Does Change of Temperature Affect Solubility Rate?

How Does Change of Agitation Affect Solubility Rate?

How Does Change of Particle Size Affect Solubility Rate?

Student Outcome –

Write a scientific explanation how temperature, particle size, and agitation affect the dissolving rate of a solute, being sure to give

proof to support your claim.

Volume of Water

Amount of sugar

Particle size

Tempera-ture of water

Agitation Time to dissolve com-

pletely

100 mL 1 tsp medium cold slow and constant

100 mL 1 tsp medium room temp

slow and constant

100 mL 1 tsp medium hot slow and constant

Volume of Water

Amount of sugar

Particle size


Agitation (stirring) Time to dissolve com-pletely

100 mL 1 tsp medium

room temp still (no agitation)

100 mL 1 tsp medium

room temp slow and constant

100 mL 1 tsp medium

room temp rapid

Volume of Water

Amount of sugar

Particle size


Agitation (stirring)

Time to dissolve com-pletely

100 mL 1 tsp small room temp slow and constant

100 mL 1 tsp medium


100 mL 1 tsp large


S1

Documents

Solutions A SOLUTION is a mixture Most water is a alloy that ...alkisites.vansd.org/dgray/Assignments/Solutions summary...Non-pure gold (less than 24K) is a solution of silver and