Gen Chem- Acids and Bases and units of concentration Flashcards
what is a lewis acid
accepts e- pair
what is a bronsted-lowry acid
donates H+
what is a lewis base
donates e- pair
what is a bronsted-lowry base
accepts H+
what is the Ka equation for acids
Ka= [H+][A-]/[HA]
what is the Kb equation for bases
Kb=[HB+][OH-]/[B]
what is true of the conjugate bases of the strongest acids
have weakest conjugate bases
pH and pOH equations
pH=-log10[H+}, pOH= -log10[OH-]
what do pH and pOH add to
pOH+pH= 14.0
water dissociation ( kw) equation
Kw= [H+][OH= 1.0x 10^-14
salts of weak acids and bases kw equation
Ka x Kb= kw
vapor pressure - raolts law
P= Po * solvent, Po= vapor pressure of solvent
osmotic pressure equation
= iMRT , i = van’t hoff factor
logarithm rules:
loga*a =
1
logarithm rules:
logaM^k=
klogaM
logarithm rules:
loga(MN)=
logaM + logaN
logarithm rules:
loga(M/N)=
logaM-logaN
logarithm rules:
10^log10(m)=
M
freezing point equation
delta Tf= iKfM
boiling point equation
delta Tb= iKbM
henderson-hasselbach equation
pH= pka + log(conj. base/conj. acid)
molarity (M) equation
M= moles of solute/ L of sln.
Molality (m) equation
m= 1 mole/ 1000g of solvent
Normality (N) meaning
1 equiv/ Liter
Of molarity, molality and normality, which concentrations are temperature dependent ?
molarity and normality
Osmolarity equation
osmoles/ L of sln
mole fraction
amt of solute (moles)/ total amount of solvent and solute (moles)
Dilution equation
miVi=mfVf
