Compare the stability of an amonia complex and ethylenediaminetetraacetate, (H2Y3-) complex with
Added by Justin M.
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- Ethylenediaminetetraacetate (EDTA, often represented as H2Y3-) is a polydentate ligand (hexadentate), capable of binding through six donor atoms (four carboxylate oxygens and two amine nitrogens). Show more…
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For the complexation reaction: M2+ + Y4- ↔ MY2- where Y4- is the EDTA anion, at which pH is the conditional stability constant of metal-EDTA complex almost equal to the thermodynamic stability constant? (Consecutive EDTA pKa values are: 2, 3, 6, 10)
David C.
In forming a chelate with a metal ion, a mixture of free EDTA (abbreviated Y4-) and metal chelate (abbreviated MYn-4) 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+ + Y4- ⇌ MYn-4 is governed by the equation K'f = ̑Y4- · Kf = [MYn-4] / ([Mn+] [EDTA]) where Kf is the association constant of the metal and Y4-, ̑Y4- is the fraction of EDTA in the form Y4-, and [EDTA] is the total concentration of free (unbound) EDTA. K'f is the conditional formation constant. How many grams of Na2EDTA · 2 H2O (FM 372.23 g/mol) should be added to 1.88 g of Ba(NO3)2 (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 ̑Y4- at pH 10.00 is 0.30. mass Na2EDTA · 2 H2O =
Supreeta N.
Which complex is more stable, $\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ or $\left[\mathrm{Cr}(\mathrm{en})_{3}\right]^{3+} ? \mathrm{Why?}^{2}$
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