Question

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 Mn+ + Y?? ? MY??? is governed by the equation K'f = ?Y?? · Kf = [MY???] / ([Mn+] [EDTA]) where Kf is the association constant of the metal and Y??, ?Y?? is the fraction of EDTA in the form Y??, and [EDTA] is the total concentration of free (unbound) EDTA. K'f is the conditional formation constant. How many grams of Na?EDTA · 2 H?O (FM 372.23 g/mol) should be added to 1.88 g of Ba(NO?)? (FM 261.35 g/mol) in a 500. mL volumetric flask to give a buffer with pBa²? = 7.00 at pH 10.00? log Kf for Ba–EDTA is 7.88 and ?Y?? at pH 10.00 is 0.30. mass Na?EDTA · 2 H?O =

          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
Mn+ + Y?? ? MY???
is governed by the equation
K'f = ?Y?? · Kf = [MY???] / ([Mn+] [EDTA])
where Kf is the association constant of the metal and Y??, ?Y?? is the fraction of EDTA in the form Y??, and [EDTA] is the total concentration of free (unbound) EDTA. K'f is the conditional formation constant.

How many grams of Na?EDTA · 2 H?O (FM 372.23 g/mol) should be added to 1.88 g of Ba(NO?)? (FM 261.35 g/mol) in a 500. mL volumetric flask to give a buffer with pBa²? = 7.00 at pH 10.00? log Kf for Ba–EDTA is 7.88 and ?Y?? at pH 10.00 is 0.30.

mass Na?EDTA · 2 H?O =

$In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y??) and metal chelate (abbreviated MY???) can buffer the free metal ion concentration at values near the dissociation constant of the metal chelate, just as a weak acid and a salt can buffer the hydrogen ion concentration at values near the acid dissociation constant. The equilibrium Mn+ + Y?? ? MY??? is governed by the equation K'f = ?Y?? · Kf = [MY???] / ([Mn+] [EDTA]) where Kf is the association constant of the metal and Y??, ?Y?? is the fraction of EDTA in the form Y??, and [EDTA] is the total concentration of free (unbound) EDTA. K'f is the conditional formation constant. How many grams of Na?EDTA · 2 H?O (FM 372.23 g/mol) should be added to 1.88 g of Ba(NO?)? (FM 261.35 g/mol) in a 500. mL volumetric flask to give a buffer with pBa²? = 7.00 at pH 10.00? log Kf for Ba–EDTA is 7.88 and ?Y?? at pH 10.00 is 0.30. mass Na?EDTA · 2 H?O =$

Added by Ricardo R.

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