-If you make up a solution of 100mL of 0.1M Hepes in the basic form, what will be the pH?
-Now you add 3mL of 1M HCl to the solution above, now what will by your pH?
-what can you conclude about the effect of dilution on the pH of a buffer?
Hepes pKa = 7.5
Hepes + H2O <-> HepesH+ + OH-
then
V = 0.1 L
M = 0.1 M
solve for
pH = -log[H+]
Kb = [HepesH+][OH-]/[HEPES]
10^-6.5 = x*x/(0.1-x)
x =1.1776*10^-4
pOH = -log(OH) = -log(1.1776*10^-4) = 3.9290
ph = 14-3.9290= 10.071
b)
if add 3 ml of 1 M Hcl then
conjugat acid = 0 + 3*1 = 3
base = 0.1*100 - 3*1 = 7
total V = 100+3 = 103
then
this is a buffer so
pOH = pKb + log(conjugate/base)
pOH = 6.5 + log(3/7) = 6.1320
ph = 14-6.1320 = 7.868
c)
change in pH
pH = 10.071-7.868 = 2.203
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