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Chapter 12: Q1 TY (page 269)

At what pH does $α_{y^{4 -}} = 0.50$ ?

Short Answer

Expert verified

At pH 10.35 the value of $α_{y^{4 -}} = 0.50$

Step by step solution

Introduction

The fraction of all free EDTA (in Y^4- format) is expressed in terms of $α_{Y^{4 -}}$ . It can be expressed as

$α_{Y^{4 -}} = \frac{[Y^{4 -}]}{[H_{6} Y^{2 +}] + [H_{5} Y^{+}] + [H_{4} Y] + [H_{3} Y^{-}] + [H_{2} Y^{2 -}] + [H Y^{3 -}] + [Y^{4 -}]}$

Given Data

In table 12-1 values of for EDTA at different pH is given.

From the above table the following graph was obtained

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Most popular questions from this chapter

Calculate the concentration of H₂Y^2- at the equivalence point in Exercise 12-C

Spreadsheet equation for auxiliary complexing agent. Consider the titration of metal M (initial concentration = C_M, initial volume = V_M) with EDTA (concentration = C_EDTA, volume added = V_EDTA) in the presence of an auxiliary complexing ligand (such as ammonia). Follow the derivation in Section 12-4 to show that the master equation for the titration is

$ϕ = \frac{C_{EDTA} V_{EDTA}}{C_{M} V_{M}} = \frac{1 + K_{f}^{''} [M]_{free} - \frac{[M]_{free} + K_{f}^{''} [M]_{free}}{C_{M}}}{K_{f}^{''} [M]_{free} + \frac{[M]_{free} + K_{f}^{''} [M]_{free}^{2}}{C_{EDTA}}}$

where $K_{f}^{''}$ is the conditional formation constant in the presence of auxiliary complexing agent at the fixed pH of the titration (Equation 12-18) and [M]_free is the total concentration of metal not bound to EDTA. [M]_free is the same as [M] in Equation 12-15. The result is equivalent to Equation 12-11, with [M] replaced by [M]_free and $K_{f}$ replaced by $K_{f}^{''}$ .

According to Appendix I, Cu²⁺ forms two complexes with acetate:

$\begin{matrix} C u^{2 +} + C H_{3} C O_{2}^{-} ⇌ C u {(C H_{3} C O_{2})}^{+} β_{1} (= K_{1}) \\ C u^{2 +} + 2 C H_{3} C O_{2}^{-} ⇌ C u {(C H_{3} C O_{2})}_{2} β_{2} \end{matrix}$

(a) Referring to Box 6-2, find K₂ for the reaction

$C u {(C H_{3} C O_{2})}^{+} + C H_{3} C O_{2}^{-} ⇌ C u {(C H_{3} C O_{2})}_{2} (a q) K_{2}$

(b) Consider 1.00 L of solution prepared by mixing 1.00 × 10^-4 mol Cu(ClO₄)₂ and 0.100 mol CH₃CO₂Na. Use Equation 12-16 to find the fraction of copper in the form Cu²⁺

Find pZn²⁺ after adding 30.0 and 51.0 mL of EDTA.

If back titration required 13.00 mL Zn²⁺, what was the original concentration of Ni²⁺?

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At what pH does αy4-=0.50?

Short Answer

Step by step solution

Introduction

Given Data

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At what pH does $α_{y^{4 -}} = 0.50$ ?