shit you don't know Flashcards
(208 cards)
Ka*Kb=
10^-14
what is water capable of doing
autoionization therefore in equilibrium ka= kw (10^-14)
pH is the logarithm of the hydronium ions
pH= -log(H3O+)
red litmus paper turns what color when it is in contact with base
blue
buffers can be
a weak acid with its conjugate base
a weak base with its conjugate acid
weak acids
HF, CH3COOH (acetic acid), HCN, HNO2, H2CO3, H2SO3, H3PO4, (COOH)2
weak base
ammonium NH3, hypochlorite ion, carbonate ion, hydrosulfide ion, methylamine, hydroxylamine, pyridine
how do buffers work
when a strong acid is added the base neutralizes the H3O+ ions
when a strong base is added the acid neutralizes the OH- ions
what is needed for a buffer to be the most effective
the number of moles of the weak acid and its conjugate base must be large and vice versa compared to the strong acid or base that is being added
buffer that maintains the blood pH
H2CO3+H2O–> HCO3-+H30+
pH of the blood is maintained around
7.4
what happens if the pH goes any lower than 6.8 or above 7.8
our cells will begin to denature
Ka is the
acid ionization constant or acid dissociation constant
Ka»>1 is a
strong acid because you will more readily ionize therefore there will be more products versus the reactants
stronger acid makes for a
weaker conjugate base
ka«<1 is a
weak acid
water is amphoteric therefore it can
act as an acid or a base
Kw is the
autoionization constant
autoionization of water equation
[H3O+][OH-]. you ignore the starting water because it is pure water
concentration of hydronium and hydroxide in water at standard temp
1*10^-7
you have such low concentration of ions in autoionization because
it is equal to 1*10^-14 making the ka very very small
ph=
-log(H3O+)
scientific notation if you have positive integer
move to the right
Scientific notation if you have negative integer
move to the left