In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y) and metal chelate (abbreviated MY") can buffer the free metal ion concentration at values near the dissociation constant of the metal chelate, just as a weak acid and a salt can buffer the hydrogen ion concentration at values near the acid dissociation constant. The equilibrium Mt + Y = MY" is governed by the equation MY K = ays - Kr = [M*] [EDTA] where K, is the association constant of the metal and Y, aya is the fraction of EDTA in the form Y, and [EDTA] is the total concentration of free (unbound) EDTA. K' is the conditional formation constant. How many grams of Na, EDTA - 2H,0 (FM 372.23 g/mol) should be added to 1.64 g of Ba(NO,), (FM 261.35 g/mol) in a 500. ml. volumetric flask to give a buffer with pBa+ = 7.00 at pH 10.00? log K, for Ba-EDTA is 7.88 and aya at pH 10.00 is 0.30.
In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y) and metal chelate (abbreviated MY") can buffer the free metal ion concentration at values near the dissociation constant of the metal chelate, just as a weak acid and a salt can buffer the hydrogen ion concentration at values near the acid dissociation constant. The equilibrium Mt + Y = MY" is governed by the equation MY K = ays - Kr = [M*] [EDTA] where K, is the association constant of the metal and Y, aya is the fraction of EDTA in the form Y, and [EDTA] is the total concentration of free (unbound) EDTA. K' is the conditional formation constant. How many grams of Na, EDTA - 2H,0 (FM 372.23 g/mol) should be added to 1.64 g of Ba(NO,), (FM 261.35 g/mol) in a 500. ml. volumetric flask to give a buffer with pBa+ = 7.00 at pH 10.00? log K, for Ba-EDTA is 7.88 and aya at pH 10.00 is 0.30.
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 79E: In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The...
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![In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y*-) and metal chelate (abbreviated MY") can
buffer the free metal ion concentration at values near the dissociation constant of the metal chelate, just as a weak acid and a salt
can buffer the hydrogen ion concentration at values near the acid dissociation constant.
The equilibrium
M+ + Y*- MY"4
is governed by the equation
MY )
[M**] [EDTA]
K = aya · Kr =
where K, is the association constant of the metal and Y, ays is the fraction of EDTA in the form Y, and [EDTA] is the total
concentration of free (unbound) EDTA. K' is the conditional formation constant.
How many grams of Na, EDTA 2 H,0 (FM 372.23 g/mol) should be added to 1.64 g of Ba(NO,), (FM 261.35 g/mol) in a
500. mL volumetric flask to give a buffer with pBa+= 7.00 at pH 10.00? log K, for Ba-EDTA is 7.88 and
at pH 10.00
is 0.30.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb2a6eecc-fc70-45a8-930d-7fdbea1bb8eb%2F78bb80ad-2521-4e78-9971-3737bd0d3fd4%2Fpt9rpk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y*-) and metal chelate (abbreviated MY") can
buffer the free metal ion concentration at values near the dissociation constant of the metal chelate, just as a weak acid and a salt
can buffer the hydrogen ion concentration at values near the acid dissociation constant.
The equilibrium
M+ + Y*- MY"4
is governed by the equation
MY )
[M**] [EDTA]
K = aya · Kr =
where K, is the association constant of the metal and Y, ays is the fraction of EDTA in the form Y, and [EDTA] is the total
concentration of free (unbound) EDTA. K' is the conditional formation constant.
How many grams of Na, EDTA 2 H,0 (FM 372.23 g/mol) should be added to 1.64 g of Ba(NO,), (FM 261.35 g/mol) in a
500. mL volumetric flask to give a buffer with pBa+= 7.00 at pH 10.00? log K, for Ba-EDTA is 7.88 and
at pH 10.00
is 0.30.
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