Part B During the reaction, 4.10 μmol of HCl are produced. Calculate the final pH of the reaction solution. Assume that the HCI is completely neutralized by the buffer. Express your answer using two decimal places. [5] ΑΣΦ w ?
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![A biochemical reaction takes place in a 1.00 mL solution of 0.0250
M phosphate buffer initially at pH = 7.37.
Acid (Proton
Donor)
H3PO4
Phosphoric
acid
H₂PO4
Dihydrogen
phosphate ion
HPO42-
Monohydrogen =
phosphate ion
Conjugate
Base (Proton
Acceptor)
H₂PO4
Dihydrogen
phosphate ion
3-
рка
PO4³-
Phosphate ion
Ka(M)
HPO42-
Monohydrogen + H+ 6.86 1.38 x 10-7
phosphate ion
+H+ 2.14 7.24 × 10-³
+ H+ 12.4 3.98 x 10-¹
-13
Are the concentrations of any of the four possible phosphate species negligible?
Check all that apply.
H3PO4
HPO42-
3-
PO4³-
H₂PO4
none of the above
Submit
Correct
3-
2-
At pH = 7.37 [H3PO4] and [PO4³-] will be negligible. The pKą of
H3PO4 = 2.14, which is ~ five pH units below 7.37. Thus, the Henderson-
Hasselbalch equation predicts that [H₂PO4¯] > [H³PO4] by five orders of
magnitude (~ 100,000 : 1) at pH 7.37. Likewise, the pKa of HPO4²- = 12.4,
which is ~ five pH units above 7.37. Thus, the Henderson-Hasselbalch equation
predicts that [HPO4²-] > [PO4³-] by five orders of magnitude (~ 100,000 : 1) at
pH 7.37.
2
3-
Part B
Previous Answers
During the reaction, 4.10 µmol of HCl are produced. Calculate the final pH of the reaction
solution. Assume that the HCI is completely neutralized by the buffer.
Express your answer using two decimal places.
pH =
VE ΑΣΦ
=
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