Science 25 LAB
Non-polar substances
-Toluene -Benzene
Polar solvent examples
-Water -Alcohol
Water surrounding dialysis bag
-barium ion present -positive for chloride ion -Starch present Conclusion small ions such barium 2+ and chloride ions easily travel through semi permeable membrane. And colloidal such as starch solution 1% does not cause its larger
Content of dialysis bag
-barium ion present -positive for starch -positive chloride ion
Silver Nitrate to test for Chloride Ion
-forms AglCl percipitate -white solid precipitated -suspension solution
Inside Dialysis Bag
-mixure of collidal solution: starch 1% -true solution: Barium Chloride, barium 2+ion and chloride CL-ion -Homogeneous mixture
Cu + 2AgNO³➡️2Ag + Cu(NO³)²
-single replacement -silver Nitrate being dissolved -copper source of electrons that will turn silver ions into silver electrons. -aqueous -does not react as fast -bluish color liquid -Pure silver solid is form -Product silver and Copper to Nitrate
moles of HCl
0.02095
2CO2 (gas)
2 carbon dioxide molecules
3O2 (gas)
3 Oxygen molecules
3H2O (liquid)
3 water molecules
Procedure to see how many moles of hcl react with tablet.
50ml of HCl -bubbles developed -5mL sodium hydroxide -boil tablets for 2 mins to get rid of all the co2 -add penaphile and then add sodium hydroxide to change color purple.
Molarity
A common measure of solute concentration, referring to the number of moles of solute per liter of solution.
Solid
A form of matter that has a definite shape and volume
Solvent
A liquid substance capable of dissolving other substances
Potential of Hydrogen (ph)
A measure of the acidity or alkalinity of a solution
Heterogeneous Mixture
A mixture in which different materials can be distinguished easily
homogeneous mixture
A mixture in which substances are evenly distributed throughout the mixture
Solution
A mixture of a solute in a solvent.
Endothermic reaction
A reaction in which energy is absorbed. -takes in heat colder outside
Exothermic Reaction
A reaction that releases energy in the form of heat -release heat colder inside than outside. example freezing and condensation
Titration
A solution of known concentration is used to determine the concentration of another solution.
liquid
A state of matter that has no definite shape but has a definite volume.
Gas
A state of matter with no definite shape or volume
Compound
A substance made up of atoms of two or more different elements joined by chemical bonds
Single Replacement reaction
A+BC➡️AC+B a chemical change in which one element replaces a second element in a compound
Alkanes
Alkanes have no functional groups.
2NH4SCN (s)
Ammonia Thiocyanate
Universal indicator
An indicator with a different colour for each pH value.
Hoffman meter
Apparatus used in lab to separate out the H2 and O2 gases from water
Suspensions
Are mixtures of finely divided substances in a suspending medium.
Frequency +light
Blue light has a higher frequency than red light.
Light+energy
Blue light has more energy than red light
Ca(O2C2H3)² (aqueous, saturated)
Calcium acetate
Ca2
Calcium ion (aq)
2H2O2 + KI ➡️ O2 + 2H2O
Catalyst reaction -catalyst potassium iodine - more production of oxygen -bubbles - faster reaction
clues that a chemical reaction has taken place
Color Change. Production of an odor. Change of Temperature. Evolution of a gas (formation of bubbles) Precipitate (formation of a solid)
CH3CH2OH + 3O2 ➡️ 2CO2 + 3H2O
Combustion reaction -creates heat and light when spark -produces CO2 and H2O
True Solutions
Contains small molecules and ions -Homogeneous mixture
Cu
Copper -good conductor
2Cl (aq)
DICHLOROPHENYL)ACETIC ACID
2PbO2 ➡️ 2PbO +O2
Decomposition reaction -releases oxygen- flame reignites. - color changed from black to orange.
2H² + O²➡️2H²O
Dihydrogen Monoxide -combination reaction -when combined with hydrogen gas from the balloon; hydrogen gas is a great source of energy, it forms a new substance water H2O when a little jolt of energy is added (heat.) -fire explosion -aqueous -loud noise -
AgNO3 + NaCl ➡️ AgCl + NaNO3K
Double Replacement reaction - Silver Nitrate and Sodium Chloride -silver Nitrate reacting with sodium Chloride. -2 cations AG+ and Na+ exchanged anions -produces AgCL(silver Chloride) (white percipitate.) and sodium Nitrate. -sodium Nitrate is soluble in water thats why you do not see it. -solid
2AgNO3 + K2CrO4 ➡️ Ag2CrO4 + 2KNO3
Double Replacement reaction -Produces silver chromate and potassium Nitrate -percipitate red color -solid - potassium Nitrate dissolved in water because its a soluble substance.
2 NaHCO3 + H2SO4 ➡️ Na2SO4 + 2H2CO3 ⬇️ H2O + CO2
Double replacement reaction -double displacement reaction because sodium changes places with hydrogen ion and forms a sodium sulphate, and carbonic acid. Which is unstable so as a result decomposes right into water and CO2 gas. -
Heat + Ba(OH)2 + 2NH4SCN ➡️ 2NH4OH + Ba(SCN)2
Endothermic Reaction -takes energy from surrounding -droplet got frozen -heat sucked in droplet got frozen as a result
CaCl2 (s) ➡️ Ca2 + 2Cl
Exothermic Reaction
Ca(O2C2H3)² + CH3CH2OH> sterno (flammable)
Gel formation (not a reaction, its a physical change) -creates gel -gel use to make sterno - burns slowly - flammable
Carbon-in the form of Charcoal change Carbon dioxide.
Glow Amber -like a fire cracker
noble gases
Helium, Neon, Argon, Krypton, Xenon, Radon
2H²
Hydrogen Peroxide
2NH4OH (aq)
Hydroxide
Water and Chloroform
Immiscible
Dialysis process
In the dialysis process solution particles are separated from colloidal particles by means of a selectively permeable membrane. -colloidal particles do not pass through a membrane. - The principle of dialysis is very important in hemodialysis in an artificial kidney machine, where certain body wastes that are dissolved in the blood are removed. -simple filtration method -semi permeable membrane
Galvanometer
Instrument used for measuring very small electrical currents
Geiger Counter
Instrument used to detect the emitted beta particles.
Iodine+Solutions
Iodine passes through the bag's semi-permeable membrane and turns Starch blue-black.
Ionic+polar substances
Ionic or polar substances dissolve in polar solvents.
Solute
Is the substance that is dissolved or goes into solutions.
2PbO2 (s, black)
Lead dioxide
2PbO (solid, orange, ppt)
Lead monoxide lead(II) Oxide
2Mg+O²➡️2MgO
MAGNESIUM OXIDE combination reaction -forms a white powder -example of an oxidation reaction reduction. -example of combination reaction. -forms a bright white/UV light -shiny turns white solid
2Mg
Magnesium Ion
metals+oxygen
Many Metals react with Oxygen to form compounds call oxides. example: iron reacts with oxygen to form iron(III) OXIDE (RUST)
Metalloids
Metalloids will also react with oxygen. Silicon forms silicon dioxide, the main component of sand, when reacts with oxygen.
Metals and No Metals with Oxygen
Metals are Basic Non- metals are acidic.
Alcohol and Chloroform
Miscible
water and ethanol/alcohol
Miscible
Why do we use Antacids
Neutalize Hydrochloric Acid in Stomach -active ingredient is CaCo3(s) Calcium carbonate. CaCO3 + CaCl2➡️ CaVl2 + H2O + CO2
Non polar+covalent
Non polar covalent substances dissolve in non polar solvent
Phosphorus ph
Orange 5
Downward displacement of water
Oxygen is collected by a method of downward displacement of water.
Oxygen
Oxygen is the most abundant element on the Earth's surface. -Earth's Atmosphere contains 21 Percent by volume of Oxygen -water bodies contains about 89% by weight of Oxygen -Earth's crust predominantly made of silica (silicone dioxide)
silicone dioxide (SiO2).
PHYSICAL PROPERTIES Main component of sand when react with oxygen brown grainy/granule Solid -when heated no color change - Sand did not change physical or chemical change
Sodium Nitrat (NaNo3)
PHYSICAL PROPERTIES -white -granule/solid -when under flames it turns liquid -liquid bubbles into gas -wooden splint reignites so there is oxygen being released
Lead Oxide (IV) PbO2
PHYSICAL PROPERTIES Black powder color changed from black to orange or a red- brown - there is oxygen being released -solid
Magnesium Oxide (MgO)
PHYSICAL PROPERTIES White powder use to make brick NO PHYSICAL CHANGE
Potassium Chlorate (KCIO3)
PHYSICAL PROPERTIES white powder -change to liquid when heated. - releases oxygen -creates like a little rocket
2KNO3 (aqueous)
Potassium Nitrate
Red Phosphorus
React with Oxygen change to P4O10 - small solid forms - bright flame
Wavelength+light
Red light has longer wavelength than blue light.
2AgNo3 (aqueous)
Silver Nitrate
2AgNO³
Silver Nitrate -colourless
2 NaHCO3 (aqueous)
Sodium Bicarbonate
Solutions+temperature
Solutions boil at a temperature that is higher than the normal boiling point of the pure solvent, and freeze at a temperature that is lower than the freezing point of the pure solvent.
Solute
Substance being dissolved
Product
The chemical composition of the result of the reaction.
Solute+temperature of solvent
The present of a solute affects the boiling point and freezing point of the solvent.
Visible Light(Tyndall Effect)
True Solutions-no light path Colloidal- red light beam
Phenolphtalein Indicator
Turn pink if the environment is basic -clear if acidic
Trough
Water bath
Test to see if iodine goes through semi permeable membrane
Yes iodine as a molecule travel though semi permeable membrane -the boiling water surrounding the dialysis bag prove that none of the starch came out because it did not turn blue.
Everytime use molarity
You have to use LITERS.
Zn
Zinc
combination reaction
a chemical change in which two or more substances react to form a single new substance. A+B➡️AB
combustion reaction
a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light 2H2(g) + O2(g) ➡️ 2H2O(g)
decomposition reaction
a reaction in which a single compound breaks down to form two or more simpler substances AB ➡️ A + B
oxidation-reduction reaction
a reaction in which electrons are transferred from one reactant to another
double replacement reaction
a reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds. AB + CD➡️ AD + CB
synthesis reaction
a reaction in which two or more substances combine to form a new compound
Simple filtration
a simple technique used to separate solid particles from suspension in a liquid solution.
suspension solution
a solution in which particles settle (sediment) -heterogeneous mixture -Usually precipitate
aqueous solution
a solution in which water is the solvent
saturated solution
a solution that cannot dissolve any more solute under the given conditions
supersaturated solution
a solution that holds more dissolved solute than is required to reach equilibrium at a given temperature
dioxide
an oxide containing two atoms of oxygen in the molecule
relative proprotions
balance equations indicates the relative proportion of each reactant and product.
Ba(OH)2 (s)
barium hydroxide
Ba(SCN)2 (aq)
barium thiocyanate
Magnesium
bluish purple
Boiling water 100 degrees celcius
boiling point of water elevated to 103.5 after adding sodium Chloride
pure solven
by50mL salt (sodium Chloride)solution used to depress the freezer point. was 1.5 now negative 1
CaCl2 (s)
calcium chloride
Reagents
chemical substances known to react in specific ways; used to detect or synthesize other substances in chemical reactions
Immiscible liquids
combinations of liquids that are incapable of mixing with, or dissolving in, each other
Diatomic
consisting of two atoms
super saturated solution
contains more dissolved solute than a saturated solution at the same temperature
O²
dioxygen
Negative beta particle
electron
CH3CH2OH (ethanol)
ethanol
CH3CH2OH (liquid)
ethanol (ethyl alcohol)
PROPERTIES OF OXYGEN
gas (colorless, odorless, tasteless), slightly heavier than air, slightly soluble in water, does not burn but will support combustion. Oxygen is a highly reactive element.
Noble Metals
gold, silver, platinum -they don't like to react
Soulution
homogeneous mixture in which one substance is evenly mixed with another substance
H2 (gas)
hydrogen gas
2H2O2 (liquid)
hydrogen peroxide
Sulfuric Acid to test for Barium ion
if barium ion is present it will form barium suphate SOLID. -white precipitation
water and toluene
immiscible
Acidic pH
less than 7 -colors: red,orange,yellow.
Miscible liquids
liquids that dissolve freely in one another in any proportion
Conservation of mass
mass cannot be created or destroyed
Triangle in Reaction
means that heat applied
Alcohol and Toluene
miscible
Chloroform and toulene
miscible
Colloidal Dispersions
mixtures containing particles larger than normal solutes but small enough to remain suspended in the dispersing medium. -Colloids do not settle out on standing.
Molarity formula
moles of solute/liters of solution
Alkaline pH/Basic
more than 7 colors:green, blue, purple
Iron ph
neutral
Ph 7 is neutral
neutral
Carbon ph
neutral 7 Sea green
percipitation reaction
occur when cations and anions in aqueous solution combine to form an insoluble ionic solid called a precipitate.
Particle of light
photon
K2CrO4 (aqueous, yellow)
potassium chromate
KI (s, white)
potassium iodide
Sulfur
react with oxygen -forms SO2 and SO3 gases -sulfur loves oxygen, bright flame when react with oxygen
Iron-steel wool
react with oxygen. -burns bright
Sulfur ph
red
AgCl
silver chloride
Ag2CrO4 (solid, red)
silver chromate
AgNO3
silver nitrate
Zn + H²SO⁴➡️ZnSO⁴ + H²
single replacement reaction (zinc sulphate) -bubbles (could be hydrogen gas, could be oxygen gas or Co2 gas.) -produce Hydrogen gas. Made a pop sound. If it was oxygen splint would be reignite. If it was Co² gas it would extinguish the flame which is one reason why Co² is in fire extinguishers.
Saturated clear solution saturated solution of sodium Acetate crystals make it supersaturated
sodium Acetate crystals added fast growth of crystals
NaCl
sodium chloride (salt)
NaNO3
sodium nitrate
Na2SO4 (aqueous)
sodium sulfate
colloidal solution
solution containing larger molecules, but not as large as suspension. -Homeogenus mixture
catalyst reaction
speed up a reaction by reducing the activation energy or changing the reaction mechanism
H2SO4 (aqueous)
sulfuric acid
H²SO⁴
sulfuric acid
Gel Formation
the formation of a gel with cooling of a gelatinized starch paste
Organic chemistry
the molecules that are predominantly made of carbon and hydrogen -occasionally oxygen, nitrogen, sulfur.
Reactants
the number and kinds of the interacting substances
chemical reaction
the process by which one or more substances change to produce one or more different substances
Oxide
the product of the reaction of oxygen with a non metal is an oxide.
instantaneous speed
the speed of an object at one instant of time. -Speedometer shows instantaneous speed.
Solvent
the substance in which the solute dissolves
oxidize
to combine with oxygen; to rust
Iodine test for starch
turns blue/black
Molecule
two or more atoms held together by covalent bonds
stoichiometric coefficients
types of numbers written infront of atoms, ion and molecules in a chemical reaction to balance them.