A biochemical reaction takes place in a 1.00 ml solution of 0.0250 Mphosphate buffer initially at pH = 7.20 (as shown for pKas of phosphatespecies).(a) Are the concentrations of any of the four possible phosphate speciesnegligible? If so, identify them and explain your answer.(b) During the reaction, 3.80 μmol of HCl are produced. Calculate the finalpH of the reaction solution. Assume that the HCl is completely neutralizedby the buffer. TABLE 2.6 Some weak acids and their conjugate basesAcid (Proton Donor)Conjugate Base (Proton Acceptor)pKaKa (M)HCOOHHCOO-+H+3.751.78 x 10-4Formic acidFormate ionCH;COOHAcetic acidCH3CO0-Acetate ion+H+4.761.74 x 10-5OHOH+H+3.861.38 x 10-4CH,CH-Co0-CH3CH-COOHLactic acidLactate ionH3PO4Phosphoric acidH,PO,Dihydrogen phosphate ion+H+2.147.24 x 10-3H,PO,Dihydrogen phosphate ionHPO,?-Monohydrogen phosphate ion+H+6.861.38 x 10-7HPO-Monohydrogen phosphate ionPO,-Phosphate ion+H+12.43.98 x 10-13H,CO3Carbonic acidHCO,-Bicarbonate ion+H+6.3*5.1 x 10-7*HCO,-Bicarbonate ionco?-Carbonate ion+H*10.255.62 x 10-11C6H5OHPhenol+H+9.891.29 x 10-10Phenolate ionNH3Ammonia+H+9.255.62 x 10-10Ammonium ion"Apparent pk, and K. values (see text for explanation).1 1

Acids dissociate into ions in the aqueous medium. The extent of dissociation determines its acidic…

Answered: TABLE 2.6 Some weak acids and their…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.62PAE: 12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c)...

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A biochemical reaction takes place in a 1.00 ml solution of 0.0250 M
phosphate buffer initially at pH = 7.20 (as shown for pK_as of phosphate
species).
(a) Are the concentrations of any of the four possible phosphate species
negligible? If so, identify them and explain your answer.
(b) During the reaction, 3.80 μmol of HCl are produced. Calculate the final
pH of the reaction solution. Assume that the HCl is completely neutralized
by the buffer.

TABLE 2.6 Some weak acids and their conjugate bases
Acid (Proton Donor)
Conjugate Base (Proton Acceptor)
pKa
Ka (M)
HCOOH
HCOO-
+H+
3.75
1.78 x 10-4
Formic acid
Formate ion
CH;COOH
Acetic acid
CH3CO0-
Acetate ion
+H+
4.76
1.74 x 10-5
OH
OH
+H+
3.86
1.38 x 10-4
CH,CH-Co0-
CH3CH-COOH
Lactic acid
Lactate ion
H3PO4
Phosphoric acid
H,PO,
Dihydrogen phosphate ion
+H+
2.14
7.24 x 10-3
H,PO,
Dihydrogen phosphate ion
HPO,?-
Monohydrogen phosphate ion
+H+
6.86
1.38 x 10-7
HPO-
Monohydrogen phosphate ion
PO,-
Phosphate ion
+H+
12.4
3.98 x 10-13
H,CO3
Carbonic acid
HCO,-
Bicarbonate ion
+H+
6.3*
5.1 x 10-7*
HCO,-
Bicarbonate ion
co?-
Carbonate ion
+H*
10.25
5.62 x 10-11
C6H5OH
Phenol
+H+
9.89
1.29 x 10-10
Phenolate ion
NH3
Ammonia
+H+
9.25
5.62 x 10-10
Ammonium ion
"Apparent pk, and K. values (see text for explanation).
1 1

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