In: Chemistry
A. At pH 7, what are the relative concentrations of ionized and un-ionized p-nitrophenol? (pKa of p-nitrophenol is 7.0)
B. If enough concentrated hydrochloric acid is added to a solution of p-nitrophenol to lower the pH from 7 to 5, what will happen to the relative concentrations of the ionized and un-ionized forms?
C. Ionized p-nitrophenol has a yellow color, while the un-ionized form is colorless. The yellow color can be measured using a spectrophotometer at 400nm. In order to determine the total amount of p-nitrophenol in a solution, would you perform the spectrophotometer reading at an acidic or basic pH? Clearly explain why?
D. A solution of p-nitrophenol at pH 8.65 was found to have an A400 of 0.470. What is the total concentration (in µM) of p-nitrophenol (ionized plus un-ionized) in the solution? The molar extinction coefficient of p-nitrophenol is 17,500 M-1cm-1 and the pKa is 7.
A. At pH 7, what are the relative concentrations of ionized and un-ionized p-nitrophenol? (pKa of p-nitrophenol is 7.0)
if pKa = 7, then expect, from the buffer eqiation
HA <-> H+ + A-
pH = pKa + log(a-/HA)
7 = 7 + log(A-/HA)
if
A- = HA, then 50% is ionized, 50% is not ionized
B. If enough concentrated hydrochloric acid is added to a solution of p-nitrophenol to lower the pH from 7 to 5, what will happen to the relative concentrations of the ionized and un-ionized forms?
note that if there is more H+ present
the next equilbirium is expected:
HA <-> H+ +A-
if H+ is added, expect much more HA (not ionized) than A- (ionized)
C. Ionized p-nitrophenol has a yellow color, while the un-ionized form is colorless. The yellow color can be measured using a spectrophotometer at 400nm. In order to determine the total amount of p-nitrophenol in a solution, would you perform the spectrophotometer reading at an acidic or basic pH? Clearly explain why?
ionized = yellow, unionized = colorless
in order to get a yello wcolor, there must be plenty of A- present ( which is yellow)
therefore, it must be basic, i.e. higher than pH >7
D. A solution of p-nitrophenol at pH 8.65 was found to have an A400 of 0.470. What is the total concentration (in µM) of p-nitrophenol (ionized plus un-ionized) in the solution? The molar extinction coefficient of p-nitrophenol is 17,500 M-1cm-1 and the pKa is 7.
Apply:
A = e*l*C
C = A/(e*l)
C = 0.47 / (17500*1) = 0.000026857 M
so
pH = pKa + log(A-/HA)
8.65 = 7 + log(0.000026857 / x)
x = 0.000026857 / (10^(8.65-7)) = 6.012*10^-7
total = 0.000026857 + 6.012*10^-7 = 0.00002745 M = 0.00002745*10^6 mM = 27.45micro M