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86 Cards in this Set
- Front
- Back
States of Matter
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Solid, Liquid, Gas
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Intermolecular Forces required to create a solid: strong or weak?
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Strong
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Intermolecular Forces required for a gas: strong or weak?
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weak
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The temperature at which liquid and solid are at equilibrium.
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Melting Point (or Freezing Point)
0° C/273.15 Kelvin |
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The temperature at which liquid and gas are at equilibrium.
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Boiling Point
100°Celsius/373.15 Kelvin |
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Enthalpy of Liquid to Solid or Gas to Liquid phase change:
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negative (-ΔΤ)
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Enthalpy of Solid to Liquid or Liquid to Gas phase change:
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positive (+ΔΤ)
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Enthalpy of Vaporization
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Amount of energy required to completely convert liquid at boiling point to gas at boiling point. There is no temperature change to the substance during vaporization.
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Enthalpy of Fusion
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Amount of energy required to completely convert a substance from a solid at melting point to a liquid at melting point. There is no temperature change during fusion.
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Enthalpy of Fusion of Water
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79.7 cal/g
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Enthalpy of Vaporization of water
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???
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Specific Heat of water
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1.00 cal/g°C
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Formula for calculating Heat in a reaction:
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Heat = mass * ΔΤ * Sp.Heat (cal/g°C)
[ΔT = T2 - T1] |
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Kinetic Molecular Theory of Gases
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-There are no attractive forces between particles of gas
-Space between gas particles is very large -The average kinetic energy of gas particles is proportional to the Kelvin temperature of the gas. -Gases experience elastic collisions with each other and the walls of the container |
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Ideal Gases
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gases that obey the kinetic molecular theory
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Pressure
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Force per unit area pushing against a surface (P = F/A)
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Units of Pressure
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Atmosphere (atm)
Millimeters of Mercury (mmHg or Torr) Pascal (Pa) Pounds per Square Inch (psi) 1 atm = 760 mmHg/Torr = 14.7 psi = 101,325 Pa |
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Pressure to Volume
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Boyle's Law
Pressue and Volume are inversely proportional (P α 1/V) PV = k (constant) or P1V1 = P2V2 |
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Volume and Temperature
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Charles' Law
Volume is Directly proportional to Temperature (VαT) V/T = k (constant) or V1/T1 = V2/T2 |
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Pressure and Temperature
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Gay-Lusacs Law
Pressure is directly proportional to Temperature (P α T) P/T = k (constant) or P1/T1 = P2/T2 |
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Combined Gas Law
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PV/T = k (constant)
or P1V1/T1 = P2V2/T2 Temperature MUST be in Kelvin! |
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moles and Volume
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Avagadro's Law
Volume is directly proportional to moles of Gas (V α n) V/n = k(constant) or V1/n1 = V2/n2 (n = # of moles of gas) |
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Ideal Gas Constant (R) using atm
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R = 0.0821 L·atm/mol·K
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Ideal Gas Constant (R) using mmHg
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R = 62.4 L·mmHg/mol·K
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Ideal Gas Law
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PV = nRT
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Dalton's Law of Partial Pressure
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the total pressure of a mixture of gases is equal to the sum of the partial pressures of the components of the mixture.
Ptotal = P1 + P2 + P3 + ... P(total)V = n(total)RT |
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STP
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Standard Temperature and Pressure
0°C (273.15 K) and 1atm (760 mmHg) |
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Standard Molecular Volume
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Volume of one mole of gas at STP
22.4L for ANY gas |
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Dipole-Dipole
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-Polar molecules are attracted to one another
-strength of the attraction is approx. 1 kcal/mol (1-2% of covalent bond strength) -tend to be liquid or solid at room temperature |
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Hydrogen Bonding
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-special kind of dipole-dipole bond
-only present when there is a lone pair of Oxygen, Nitrogen, or Flourine present and a Hydrogen bonded to another O, N or F -stronger than dipole-dipole (1 kcal/mol) |
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London Dispersion Forces
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-all molecules have this (temporary dipoles)
-results from a temporary polarity caused by the random motion of electrons in a molecule -STRONGEST force experienced by NON-POLAR molecules, weakest of intermolecular forces |
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Intermolecular Forces in order or strength
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Ionic
Non-Polar Covalent Hydrogen Bonding Dipole-Dipole London Dispersion |
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Vapor Pressure
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The partial pressue of gas molecules in equilibrium with liquid. Increases with temperature.
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Relation of Boiling Point to pressure
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Directly proportional. BP decreases with lower pressure, increases with higher pressure.
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Heterogenous Mixture
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A non-uniform mixture with regions of different composition
-murky or opaque -particles often settle or can be filtered -ex. orange juice, house paint |
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Homogenous Mixture
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Uniform mixture throughout
-Homogenous solution: particles are small, solution is transparent -Homogenous colloids: larger particles, murky or opaque |
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Solute
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The dissolved substance
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Solvent
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The substance (usually liquid) the solute is disolved in.
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Solution
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Solute + Solvent
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Solubility
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maximum amount of a substance that will dissolve in a solvent at a given temperature.
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Solvation
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How a solid dissolves in a liquid.
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Solvation / Hydration
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the solvent is water
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Like dissolves Like
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Liquids with similar intermolecular forces will form solutions. Polar compounds dissolve easily in water. Non-polar compounds dissolve in non-polar liquids.
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LeChatlier's Principle
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increase in stress on one end of a system in equilibrium will result in a shift to the side of the system with fewer molecules to relieve the stress and restore equilibrium.
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Solubility and Pressure
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Solubility is Directly proportional to Pressure.
C/P = k (constant) or C1/P1 = C2/P2 (C = solubility) |
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Formula for calculating Molarity of a solution:
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M = moles of solute/Liters of solution
(mol/L) |
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Formula for calculating Weight/Volume %
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W/V% = g of solute/mL of solution x 100
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Formula for calculating Volume/Volume %
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V/V% = volume of solute/volume of solution x 100
(units must be the same!) |
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Formula for calculating Parts per Million by weight.
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PPM = Mass of solute/mass of solution x 10E6
(units must be the same) |
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Formular for calculating parts per million by volume
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PPM = volume of solute/volume of solution x 10E6
(units must be the same) |
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Formula for Dilution
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M1 x V1 = M2 x V2
M1 = original concentration (Molarity) V1 = initial volume M2 = desired concentration (Molarity) V2 = final total volume V2-V1 = amount of solvent required for dilution |
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Solid Hydrates
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ionic compounds that hold water molecules "trapped" in their lattice.
ex. Epsom Salt, MgSO4 · 7H2O (each molecule of MgSO4 holds 7 water molecules) |
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Electrolytes
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An substance that conducts electricity when dissolved in water.
STRONG ELECTROLYTES: ionic salts, strong acids & bases WEAK ELECTROLYTES: weak acids & bases, non ionic compounds, substances that don't dissolve completely in water NON ELECTROLYTES non-soluable ionic compounds |
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Equivalents of Electrolytes
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Units used to describe the amount of ions in bodily fluid.
Eq = molar mass of ions(g)/# of charges on the ion mEq = 1 Eq/1000 |
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The colligative propertives of a solution depend on the ______ rather than the identity of the solute.
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Concentration
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The presence of a solute _______ the vapor pressure of the solution.
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Lowers.
Fewer solvent molecules can escape from the solution surface into the gas phase. |
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The presence of a solute _______ the Boiling Point of the solution.
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RAISES
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The presence of a solute ______ the freezing point of a solution.
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Lowers
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What determines which solutes will have the greatest effect on the colligative properties of the solution?
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Number of particles they dissolve into. The more particles, the higher the HP/lower the MP.
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In osmosis, solvent particles always pass from an area of ______ concentration to an area of _______ concentration?
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Lower to Greater
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Osmolarity
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The sum of all the molarities in the solution.
0.10 NaCl = 0.20 osmol |
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What is the auto-ionization of water?
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Liquid water dissociates VERY SLIGHTLY into [H30+] and [OH-] ions.
H2O(l) + H2O(l) <---> H3O+(aq) + OH-(aq) Forward reaction IS NOT favored. |
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Equilibrium Constant of Water
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Kw = [H3O+] x [OH-] = 1.00 x 10E-14
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Acid
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Any substance that produces H3O+ ions when added to water.
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How to calculate concentration of an acid from the pH.
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H3O+ = 10E-pH
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How to calculate pH from the contration of the acid.
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pH = -log[H3O+]
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Sig Figs for pH
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Count the number of sig figs for pH AFTER the decimal point only.
ex. H3O+ - 2.00 x 10E-4 (3 sig figs) pH = 3.699 (3 sig figs AFTER decimal) |
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How to calculate [OH-] concentration from [H3O+] concentration
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[OH-] = 1.00 x 10e-14/[H30+]
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How to calculate [OH-] concentration from pH?
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First get [H3O+] concentration:
10e-pH = [H3O+] Then use equilibrium constant: [OH-] = 1.00 x 10e-14/[H3O+] |
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acid/base indicators
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--molecules that change color depending on the amount of [H3O+] present
--pH paper, paper coated with universal indicator gives approx pH. --pH meter, electrodes which measure actual pH |
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Definition of Acid (Arrhenius)
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A substance that provides [H3O+] ions when dissolved in water.
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Definition of Base (Arrhenius)
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a substance that provides [OH-] ions when dissolved in water.
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Definition of Acid (Bronsted-Lowry)
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a substance that donates an H+ ion.
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Definition of Base (Bronsted-Lowry)
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A substance that accepts an H+ ion (donates an electron.) MUST HAVE a lone pair of electrons.
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Formula for conjugate acids/bases
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B: + HA --> BH+ + :A-
B: is the original base HA is the original acid BH+ is the conjugate acid of B: :A- is the conjugate base of HA |
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Strong Acids
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complete dissociated
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Weak Acids
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do not dissociate completely, reactions are reversible.
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Conjugate bases of Strong acides are _______ bases.
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WEAK
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Conjugate bases of weak acides are ______ bases.
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Stronger
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The Six Strong Acids
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HCIO4 - Perchloric Acid
H2SO4 - Sulfuric Acid NHO3 - Nitric Acid HI - Hydroiodic Acid HBr - Hydrobromic Acid HCl - Hydrochloric Acid (all other acids are considered weak) |
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The Strong Bases
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Group I and II cations + OH-
(NaOH, KOH, Mg(OH)2, CA(OH)2) all other bases are considered weak. |
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Polyprotic Acids
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Acids that have more than one H+ to donate. Each subsequent dissociation will be a weaker reaction.
Ex. H2SO4 is a DIPROTIC acid H2SO4 + H2O --> H3O+ + HSO4- HSO4- + H2O <--> H3O+ + SO4-2 |
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Other important Acid/Base reactions:
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Acid + metal hydroxide = salt + water
Acid + Carbonate/bicarbonate ion --> carbonic acid --> CO2 + H2O Acid + NH3 --> ammonium salt(aq) |
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Titration
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a procedure for determining the concentration of an acid or base. A known concentration of an acid/base is added to an unknown concentration of a base/acid until pH is neutral. The amount of known substance will equal the concentration of the unknown substance.
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Another word for H3O+
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Hydronium ion
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Another word for OH-
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Hydroxyl ion
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