PHOSPHATE BUFFER PRACTICAL Flashcards
WHAT IS A BUFFER?
solution that prevents a drastic pH chage
-consists of a conjugate pair -> acid and conjugate base or base and conjugate acid
-weak acid - salt = negative ion (conjugate base)
-weak base - salt = positive (conjugate acid)
-2 different salts of the same polyprotic acid
-an amphoteric electrolyte (protein)
WHAT ARE THE MOST IMPORATANT BUFFERS IN THE HUMAN BODY?
-carbonate, phosphate, hemoglobin
WHAT ARE BUFFERS USED FOR IN THE LAB?
buffers are used to prepare solutions of known stable pH - they are used as standard solutions to calibrate pH meter or help maintain pH of some reaction mixtures
WHAT DO PROTONS REACT WITH?
conjugate base
WHAT DO HYDROXIDE IONS REACT WITH?
conjugate acid
WHAT HAPPENS WHEN AN ACID IS ADDED TO THE SOLUTION?
most of the extra protons are removed / neutralized by the base
WHAT HAPPENS WHEN A BASE IS ADDED TO THE SOLUTION?
most of the extra hydroxide ions are removed by a reaction with undissociated acid
WHAT IS THE BEST RATIO FOR A BUFFER?
ratio 1:1 of the conjugate pair is the most efficient for handling the addition of either a base or an acid
-> If the buffer contains much
more conjugate acid than conjugate base, it is less efficient in handling in acid. Alternatively, a buffer with much more of the conjugate base than of conjugate acid cannot efficiently counteract the addition of a base.
For example, the H2CO3 / HCO3
- buffer in blood has a 1:20 ratio of acid to its conjugate base. Blood is then more effective in counteracting acids, which are the products of metabolism
ACIDIC BUFFER CALCULATION
pH = pKa + log (csalt/cacid)
BASE BUFFER CALCULATION
pOH = pKb + log (csalt/ cbase)
pH = 14 - pOH
WHAT IS pKa?
negative common logarithm of the dissociation constant of the acid (pKa = - log Ka)
WHAT IS Ka?
an equilibrium constant describing a dissociation of the acid: HA <–> H+ + A-
(i.e. Ka is andissociation constant of the acid)
WHAT IS pKb
negative common logarithm of the dissociation constant of the hydroxide (pKb = - log Kb)
WHAT IS Kb?
an equilibrium constant describing a dissociation of the hydroxide: BOH B+ + OH-
(i.e. Kb is an dissociation constant of the hydroxide)
WHAT IS THE MOST EFFICIENT BUFFER?
pH = pK (the ratio of concentrations is 1/1 because log(1/1) = 0), sufficient efficiency is found if a buffer pH = pK ± 1 (it is related to the ratio of 1/10 or 10/1)
ACIDIC BUFFER WITH MOLAR CONCENTRATION
pH = pKa + log (c´salt x Vsalt / c´acid x Vacid)
BASIC BUFFER WITH MOLAR CONCENTRATION
pOH = pKb + log (c´salt x Vsalt / c´base x Vbase)
pH = 14 - pOH
WHAT IS THE CAPACITY OF A BUFFER?
the substance amount of acid or base it must be added into the buffer to change its pH by 1 pH unit (substance amount of acid or base divided by related pH change).
-buffer has its highest capacity at equal concentrations of weak acid and conjugate base, when p H = p K a
-to increase capacity -> increase total concentration