During the reaction, 4.90 μmol of HCl are produced. Calculate the final pH of the reaction solution. Assume that the HCl is completely neutralized by the buffer.

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During the reaction, 4.90 μmol of HCl are produced. Calculate the final pH of the reaction solution. Assume that the HCl is completely neutralized by the buffer.
 
Express your answer using two decimal places.
A biochemical reaction takes place in a 1.00 mL solution of 0.0250
M phosphate buffer initially at pH = 7.24.
Acid (Proton
Donor)
H3PO4
Phosphoric
acid
H₂PO4
Dihydrogen
phosphate ion
2-
HPO4²
Monohydrogen
phosphate ion
Conjugate
Base (Proton
Acceptor)
H₂PO4
Dihydrogen
phosphate ion
2-
pKa K₂(M)
PO4³-
Phosphate ion
+ H+ 2.14 7.24 × 10-³
HPO4²
Monohydrogen +H+ 6.86 1.38 x 10-7
phosphate ion
+ H+ 12.4 3.98 × 10-13
Part A
Are the concentrations of any of the four possible phosphate species negligible?
Check all that apply.
ⒸHPO4²-
PO4³
H₂PO4
✔ H3PO4
Submit
2-
3-
Onone of the above
Part B
Correct
At pH = 7.24 [H3PO4] and [PO4³-] will be negligible. The pK₁ of H3PO4 = 2.14, which is ~ five pH
units below 7.24. Thus, the Henderson-Hasselbalch equation predicts that [H₂PO4¯] > [H3PO4] by five
orders of magnitude (~100,000 : 1) at pH 7.24. Likewise, the pK₂ of HPO4²- = 12.4, which is ~ five pH
units above 7.24. Thus, the Henderson-Hasselbalch equation predicts that [HPO4²¯] > [PO4³-] by five
orders of magnitude (~ 100,000 : 1) at pH 7.24.
pH =
Previous Answers
During the reaction, 4.90 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.
15| ΑΣΦ
VL
?
Transcribed Image Text:A biochemical reaction takes place in a 1.00 mL solution of 0.0250 M phosphate buffer initially at pH = 7.24. Acid (Proton Donor) H3PO4 Phosphoric acid H₂PO4 Dihydrogen phosphate ion 2- HPO4² Monohydrogen phosphate ion Conjugate Base (Proton Acceptor) H₂PO4 Dihydrogen phosphate ion 2- pKa K₂(M) PO4³- Phosphate ion + H+ 2.14 7.24 × 10-³ HPO4² Monohydrogen +H+ 6.86 1.38 x 10-7 phosphate ion + H+ 12.4 3.98 × 10-13 Part A Are the concentrations of any of the four possible phosphate species negligible? Check all that apply. ⒸHPO4²- PO4³ H₂PO4 ✔ H3PO4 Submit 2- 3- Onone of the above Part B Correct At pH = 7.24 [H3PO4] and [PO4³-] will be negligible. The pK₁ of H3PO4 = 2.14, which is ~ five pH units below 7.24. Thus, the Henderson-Hasselbalch equation predicts that [H₂PO4¯] > [H3PO4] by five orders of magnitude (~100,000 : 1) at pH 7.24. Likewise, the pK₂ of HPO4²- = 12.4, which is ~ five pH units above 7.24. Thus, the Henderson-Hasselbalch equation predicts that [HPO4²¯] > [PO4³-] by five orders of magnitude (~ 100,000 : 1) at pH 7.24. pH = Previous Answers During the reaction, 4.90 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. 15| ΑΣΦ VL ?
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