Biochemistry
8th Edition
ISBN: 9781464126109
Author: Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr., Lubert Stryer
Publisher: W. H. Freeman
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Question
Chapter 1, Problem 17P
Interpretation Introduction
Interpretation:
The ratio of protonated to deprotonated form of acid is to be determined.
Concept introduction:
The ratio of protonated to de protonated form of an acid can be determined by the use of following expression,
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What are the components of a lysine buffer at pH 9.2? Refer to the
following forms of lysine:
A
H
B
H
H
H
H;N-C-COOH
H;N-C-coo-
H,N-C-c0-
H,N-C-coo-
CH2
CH2
CH2
CH.
CH2
CH,
pk-2.17
pk=4.04
pk=12.48
CH,
CH,
ÇH2
CH,
CH.
CH,
CH,
CH.
CH,
CH,
NH,
NH,
NH,
NH,
. A and B
.C and D
.B and C
. A and D
B and D
A 0.200 M solution of a weak monoprotic acid (HA) has a pH of 2.35. What
is the value of K of this acid?
a
K
=2.011e-4
a
What is the percent ionization of this acid?
Percent Ionization = .10
%
pH of solution
14.00
12.00
10.00
8.00
6.00
First
4.00
equivalence
point
2.00
0
First midpoint
Second
equivalence
point
Third midpoint
pH = pKa=12.32
Third
equivalence
point
HPO4(aq) + OH(aq) PO4(aq) + H2O(1)
Second midpoint
pH = pKa = 7.21
H2PO4 (aq) + OH(aq) HPO42 (aq) + H2O(1)
Using the Henderson-
Hasselback equation, show how to create
2L of a 0.1 M KPhos pH 7.5 buffer using
K2HPO4 and KH2PO4.
The chart to the left should help you
understand what pKa to start with. Show
your work.
pH = pKa = 2.16
H3PO4(aq) + OH(aq)
H2PO4(aq) + H2O(l)
25.0
50.0
75.0
100.0
Volume of NaOH added (mL)
Chapter 1 Solutions
Biochemistry
Ch. 1 - Prob. 1PCh. 1 - Prob. 2PCh. 1 - Prob. 3PCh. 1 - Prob. 4PCh. 1 - Prob. 5PCh. 1 - Prob. 6PCh. 1 - Prob. 7PCh. 1 - Prob. 8PCh. 1 - Prob. 9PCh. 1 - Prob. 10P
Ch. 1 - Prob. 11PCh. 1 - Prob. 12PCh. 1 - Prob. 13PCh. 1 - Prob. 14PCh. 1 - Prob. 15PCh. 1 - Prob. 16PCh. 1 - Prob. 17PCh. 1 - Prob. 18PCh. 1 - Prob. 19PCh. 1 - Prob. 20PCh. 1 - Prob. 21PCh. 1 - Prob. 22PCh. 1 - Prob. 23PCh. 1 - Prob. 24PCh. 1 - Prob. 25PCh. 1 - Prob. 26PCh. 1 - Prob. 27PCh. 1 - Prob. 28PCh. 1 - Prob. 29P
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, biochemistry and related others by exploring similar questions and additional content below.Similar questions
- The pKas of two hypothetical organic acids are given below. ACOOH ----> ACOO- + H+ (pKa = 4.15) BCOOH -----> BCOO- + H+ (pka = 4.55) by: The pH at which BOTH these acids will be soluble can be given OpH 4.55 4.15arrow_forwardA compound has a pKa of 7.4. You have made up 100 mL of a 1.0 M solution of this compound at pH 8.0. What is the ratio of unprotonated to protonated forms of the molecule? 80% ○ 66.7% 100% ○ 50% ○ 20%arrow_forwardCalculate the salt to acid ratio ([Aˉ]/[HA]) of a solution of an amino acid at pH 2 and pKa of 8.95arrow_forwardIf an aqueous solution has a hydroxyl ion concentration of 1 × 10-6 M, what is the concentration of hydrogen ion ([H+]) ? [H+] = 1.0 x10-5 Marrow_forwardWhat is the pH of a buffer of a buffer system that contains a weak acid of .19 M and conjugate base of .12 M ? The Ka of the acid is 5.6x 10 -6 pH= pKa + log ( [A- ]/[HA]) please show me step by steparrow_forward(E) Consider an amino acid that has one -amino group (pKa = 9.2), one -carboxyl group (pKa = 1.7) and one ionizable side chain (pKa = 6.2). At which pH range/s would this amino acid be effective as a buffer? If the amino acid shows a net charge of -1 at pH 11 and a net charge of +1 at pH 4, what pKa values would you use to calculate the isoelectric point? At what pH would the net charge be equal to zero?arrow_forwardWhat mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.arrow_forwardWhat is the pH of an aqueous solution with {H3O+} = 6x10-12arrow_forwardCalculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pKa 5 4.76) of (a) 2:1; (b) 1:3.arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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