🥰 Flashcards
Normal neural binary acids
H - hydro
Then end in ic
Polyatomic anions
H- nothing
If ion ends in ate then ic acid
If ion ends in ite then us acid
Arrhenius acid and base
Acid : increases h+
Base : increases OH-
Equation
Acid : HNO3 -> H+ + NO3-
Base : NaOH -> Na+ + OH-
Acid + base —> water + salt
HCl + NaOH —-> H2O + NaCl
Bronsted Lowry acid and base
Acid : proton donor
Base: proton acceptor
Equation
Hcl+ H2O —> H3O + cl-
Reaction doesn’t need to happen in water
A reaction with water is called hydrolysis
How to write neutralization reaction containing an acid and base containing oh-
Forms water and a salt
Titrant
Reagent of known concentration
Titration
Titration
A chemical reaction used to determine the exact amount of a reagent
Titrant is carefully added to a known volume of analyte to find the equivalence point which can be used to find the concentration
Analyte
Reagent of unknown concentration
Equivalence point
Equivalence point is when all the analyte has been reacted with the Titrant
Purpose of indicator
Is to determine the equivalence point
Turns colors to know that the reaction is done
Strong acids
HCl Hbr HI HNO3 H2SO4 HCLO4 HCLO3 Are irreversible and completely dissociate
Strong bases
LioH NaOH KOH RbOH CsOH
Strong and weak acid or base
Strong acid / base completely separates when places into a solution
Equilibrium constant for acid or base
Ka(acid) = (h30)(products)/reactants
Don’t include water !!!!!
Ka * Kb= 1x10^-14
Kw
Auto ionization of water
H20 + H2O -> H3O + OH
Kw= H3O x OH-= 1.0 x10^-14
Ph scale and calculations
pH=-log (H3O) H+= 10 ^-pH pOH= -log(OH) OH= 10^-pOH pH + pOH= 14 H+ x OH- = 1x10-14
Increase of 1 ph = 10 x increase of h+
Ph and pOH = 7 is neutral
pH<7 acidic pOH>7
pH>7 basic pOH<7
2 components of the buffer
Weak acid and conjugate base (in the form of a soluble salt)
Resistís dramatic changes in pH
Intermolecular forces
London dispersion factor
Dipole dipole
Hydrogen binding
London - all molecules (vanderwalls) induced dipole (larger the stronger)
Dipole dipole - only polar molecules
Permanent dipoles
Hydrogen binding :H bound to O N or f atom and interact with one of the 3
London < dipole < hydro
Melting and boiling point trends
The stronger the IMF the higher the melting / boiling point
If it a positive number it is endothermic
If it is negative it would be exothermic
Fusion
Melting
Solid to liquid
Solidification
Freezing
Liquid to solid
Vaporization
Liquid to gas
Condensation ☁️
Gas to liquid
Sublimation
Solid to gas (dry ice)
Deposition
Gas to solid
Heat of fusion
Delta Hfus = amount of energy needed to change from a liquid to a solid
Appeintly there is a direct correlation between enthalpy of fusion and the streagth of the imfs
Heat of vaporization
Delta H Vap amount of energy needed. For a liquid to become a gas
Increase with increase IMF for both
Hearing and cooling curve
Draw out know
Trends as energy increases heat also increases if it is not in a transition state if at a transition state energy is being used to transition meaning heat will platou
Exothermic vs endothermic
Right to left is endothermic
Left to right is exothermic
Acids vs bases characteristics
Acids Turn litmus red Give off h2 gas with some metals React with carbonate and bicarb salts to give off co2 Have a sour taste
Bases
Turn litmus blue
Are slippery to the touch
Have a bitter flavor
Conjugate acid base pare
Differ only by one proton
H20 acid OH conjugate base
Water is amphiprotic meaning it can be an acid or a base
Delta h sub
Enthalpy of sublimation
Is the energy needed to take a solid to a gas and is equal to delta h fus + delta h vap
