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Unit 3-4 notes pages 100-127
Kinetic Energy- energy an object has due to its motion
Temperature- measure of average kinetic energy of the particles in a material
Potential energy- stored energy due to interaction between particles or objects
Thermal Energy- result of the motion of all particles and the distance and attractions between those particles in the system
Atom- small particle that is the building block of matter
Substance- Matter with composition that is always the same
Element- substance made of only one type of atom
Compound- a type of substance that occurs when atoms of two or more different elements are bonded together
Chemical Formula- group of chemical symbols and numbers that represent the elements and number of atoms
Acid= A substance that produces Hydrogen ions (H+1) in a water solution. (Below 7 on the pH scale.)
Properties of acids
Have a sour taste.
Produces hydrogen ions (H+1) in solution.
Acids are corrosive-causing painful burns.
React with metal to produce H2 gas.
Change litmus paper red.
Hydronium ions=
Ion formed by bonding a Hydrogen ion (H+1), to a water molecule to give H3O+1.
Indicators=
Substances that change color as the pH of the sample changes.
*Indicator paper(pH paper)=
A strip of paper that has been coated with a combination of indicators, and they change to different colors at different pH levels.
(Special paper that changes color at different pH levels)
*pH meter=
A device that measures the pH value electronically.
Base=
A substance that forms Hydroxide ions (OH-) in water. (Bigger than 7 on the pH scale.)
Properties of bases
Have a bitter taste.
Produces hydroxide ions (OH-1) in solution.
Bases are corrosive-causing painful burns.
Bases feel slippery.
Change litmus paper blue.
*Neutral=
A substance that forms Hydroxide ions (OH-) and Hydrogen ion (H+1) in water. (Exactly 7 on the pH scale.)
* Hydroxide ions (OH-) = Hydrogen ion (H+1)
Dissociation of Acids=
Acids dissociated(separate) in water to form Hydronium ions H3O+1 or H+1.
Dissociation of Bases=
Bases dissociated(separate) in water to form Hydroxide ions (OH-).
Strong Acid=
Nearly all of the H1+ ions dissociated(separate).
Weak Acid=
Only a few of the H1+ ions dissociated(separate).
Strong Base=
Nearly all of the OH1- ions dissociated(separate).
Weak Base=
Only a few of the OH1- ions dissociated.
Dilute=
A small amount of acid or base is dissolved in water.
Concentrated=
A large amount of acid or base is dissolved in water.
pH=(Potential Hydrogen)
A measurement of the concentration of H1+ ions in a substance.
pH scale=
A range of numbers from 1-14 that show the relative H1+ ions in a substance.
Talk about the difference on the pH scale.
*Notes added for problems**
pOH =Potential Hydroxide=
Measurement of Hydroxide in a substance.
[H3O+1] = [H+1] =Hydronium ion concentration.
[OH-1] =Hydroxide ion concentration.
pH + pOH =14
[H+1][OH-1] =1 X 10-14
[OH-1] =1 X 10-pOH
[H+1] =1 X 10-pH
Problems-
Calculate the pH, pOH, [H+]and [OH-]
Ex. pOH = 2
pOH = 2
pH + pOH =14 therefore pH=14 - pOH
pH = 14-2=12
[H+] = inverse log of 12 = 1 X 10-12.
[OH-]= inverse log of 2 = 1 X 10-2
pH is more than 7, so it is a base.
If the pH is LESS than 7 it is an acid.
If the pH is MORE than 7 it is a BASE.
If the pH is EQUAL to 7 it is neutral.
Buffers=
Mixtures that resist change to the pH even when strong acids and bases are added.
*They usually contain weak acids and their conjugate base.
Neutralization= Neutralization rx-
A process in which acids are added to bases or vice versa to get the pH to 7.
(Getting acids or bases to 7.)
*This process produces salt water.
*Equivalent point(stoichiometric point)=
This results when the substances are neutralized in the titration reaction.
Salt=
A compound produced in a neutralization reaction. (Usually made of a metal and a nonmetal.)
Titration-
A process in which a known concentration of a base is added to an unknown concentration, or known volume of an acid to determine the concentration of the unknown. (Or vice versa.){A process of neutralization.}
Titration problems-Example
i.e. What is the concentration if 50 ml of 2 m base is added to 100 ml of acid?
Concentration of acid(volume of acid)= Concentration of base(volume of base) CAVA=CBVB
(CA) 100 ml = 2 m(50ml)
100ml 100ml
CA= 1 m
*Standard solution=
The acid/base with the known concentration.
*Titration curve(pH curve)=
A plot of the results of a neutralization reaction.
Soaps=Organic salts.
*Conjugate Acid= Generally a weak acid formed as a strong base accepts a hydrogen ion or proton.
*Conjugate base= Generally a weak base formed as a strong acid donates a hydrogen ion or proton.
Acids and Bases are reactants
Conjugate acids and conjugate bases are products
H-OH = H2O
*FOLLOW THE ANION(NEGATIVE PARTICLE)
Ex. HCl + NaOH à NaCl + H-OH
Acid Base Conjugate Conjugate
Base Acid
Think
ACIDS-AWAY Acids give H’s away
BASES- BRING IN H’s.
*Monoprotic Acids=
Acids with only one Hydrogen or proton. Ex. HCl
*Diprotic Acids=
Acids with two Hydrogen or proton. Ex. H2SO4
*Triprotic Acids=
Acids with three Hydrogen or proton.Ex. H3PO4
*Oxyacids=
Acids in which the acidic hydrogen is attached to an oxygen atom. (Contain Oxygen)
*Usually strong acids.)
Ex. H3PO4
*Amphoteric substances=
A substance that can act either as an acid or base.
EX. Water
*Ionization of water=
A process in which the protons of one molecule of water are transferred to another.(Water forms ions)
H2O à H+1 + OH-1
or
H2O + H2O à H3O+1 + OH-1
Kw= The Ion-Product constant of water.
Kw= [OH-1] [H+1]= 1 X 10-14
*Acid precipitation=
Any form of precipitation having a pH lower than 5.6.
*Models of Acid/Base pairs
A) Arrhenius model
Acid- These produce H+ ions in water.
Base- These produce OH- ions in water.
B) Bronsted-Lowry model
Acid- These are proton/Hydrogen donors.
(Give AWAY Hydrogens.)
Base-These are proton/Hydrogen ion acceptors.
(BRING in Hydrogens.)
C) Lewis model
Acid- These are electron acceptors.(All vowels)
Base-These are electron donors.
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