Problem 2.20 -Enhanced - with Solution 59 of Correct At pH 7.06 H PO4] and[PO will be negligible. The pKa of H3 PO 2.14, which is five pH units below 7.06. Thus, the Henderson-Hasselbalch equation predicts that H2 PO4H3PO by five orders of magnitude(100,000: 1) at pH 7.06. Likewise, the pKa of HPO4212.4, which is~five pH units above 7.06. Thus, the Henderson-Hasselbalch equation predicts that HPOP43by five orders of magnitude(100,000: 1) at pH 7.06 Review| Constants | Periodic Table A biochemical reaction takes place in a 1.00 mL solution of 0.0250 M phosphate buffer initially at pH 7.06 Acid (Proton Donor) Conjugate Base (Proton Acceptor) pKaKa(M) H3PO4 PhosphoricDihydrogen H+2.14 7.24 x 103 acid H2PO4 phosphate ion HPO2 phosphate ion PO4 3- Part B H2PO4 DihydrogenMonohydrogen +H 6.86 1.38 x 10-7 phosphate ion During the reaction, 3.40 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 HPO2 Monohydrogen Phosphate ion phosphate ion +H 12.4 3.98 x 10-13 pH- Submit Request Answer
Basics in Organic Reactions Mechanisms
In organic chemistry, the mechanism of an organic reaction is defined as a complete step-by-step explanation of how a reaction of organic compounds happens. A completely detailed mechanism would relate the first structure of the reactants with the last structure of the products and would represent changes in structure and energy all through the reaction step.
Heterolytic Bond Breaking
Heterolytic bond breaking is also known as heterolysis or heterolytic fission or ionic fission. It is defined as breaking of a covalent bond between two different atoms in which one atom gains both of the shared pair of electrons. The atom that gains both electrons is more electronegative than the other atom in covalent bond. The energy needed for heterolytic fission is called as heterolytic bond dissociation energy.
Polar Aprotic Solvent
Solvents that are chemically polar in nature and are not capable of hydrogen bonding (implying that a hydrogen atom directly linked with an electronegative atom is not found) are referred to as polar aprotic solvents. Some commonly used polar aprotic solvents are acetone, DMF, acetonitrile, DMSO, etc.
Oxygen Nucleophiles
Oxygen being an electron rich species with a lone pair electron, can act as a good nucleophile. Typically, oxygen nucleophiles can be found in these compounds- water, hydroxides and alcohols.
Carbon Nucleophiles
We are aware that carbon belongs to group IV and hence does not possess any lone pair of electrons. Implying that neutral carbon is not a nucleophile then how is carbon going to be nucleophilic? The answer to this is that when a carbon atom is attached to a metal (can be seen in the case of organometallic compounds), the metal atom develops a partial positive charge and carbon develops a partial negative charge, hence making carbon nucleophilic.
Part B of that question in the image. Please, thank you.
![Problem 2.20 -Enhanced - with Solution
59 of
Correct
At pH 7.06 H PO4] and[PO will be negligible. The pKa of H3 PO 2.14, which is
five pH units below 7.06. Thus, the Henderson-Hasselbalch equation predicts that
H2 PO4H3PO by five orders of magnitude(100,000: 1) at pH 7.06. Likewise, the
pKa of HPO4212.4, which is~five pH units above 7.06. Thus, the Henderson-Hasselbalch
equation predicts that HPOP43by five orders of magnitude(100,000: 1) at pH
7.06
Review| Constants | Periodic Table
A biochemical reaction takes place in a 1.00 mL solution of 0.0250
M phosphate buffer initially at pH 7.06
Acid (Proton
Donor)
Conjugate
Base (Proton
Acceptor)
pKaKa(M)
H3PO4
PhosphoricDihydrogen H+2.14 7.24 x 103
acid
H2PO4
phosphate ion
HPO2
phosphate ion
PO4 3-
Part B
H2PO4
DihydrogenMonohydrogen +H 6.86 1.38 x 10-7
phosphate ion
During the reaction, 3.40 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
HPO2
Monohydrogen Phosphate ion
phosphate ion
+H 12.4 3.98 x 10-13
pH-
Submit
Request Answer](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2e7a73d-22fe-4d0b-8e9e-c8fe6b88449f%2F46b82f25-4527-4dd0-b3cc-e082e099919b%2Fbqsvw88.png&w=3840&q=75)
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