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## Q. 14-5

Preparing a Metal Ion Buffer

What concentration of EDTA should be added to 0.010 M $CaY^{2−}$ at pH 6.00 to give $[Ca^{2+}]$ = 1.0 × $10^{−6}$ M?

## Verified Solution

From Equation 14-17, we write

$K_{f} = 10^{10.65} = \frac{[CaY^{2−}]}{[Ca^{2+}]α_{Y^{4−}}[EDTA]}$       (14-17)

$[EDTA] = \frac{[CaY^{2−}]}{K_{f}α_{Y^{4−}}[Ca^{2+}]} = \frac{0.010}{(10^{10.65})(1.8 × 10^{−5})(1.00 × 10^{−6})} = 0.012_{4}$ M

These are practical concentrations of $CaY^{2−}$ and of EDTA.

Test Yourself      What concentration of EDTA should be added to 0.010 M $CaY^{2−}$ at pH 6.00 to give $[Ca^{2+}]$ = 1.0 × $10^{−7}$ M? (Answer: $0.12_{4}$ M)