Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions. A 27.50 mL sample of 0.0652 M Ni²+ was added to 27.50 mL of 0.195 M iminodiacetic acid (the completely protonated form is abbreviated as H3A+) buffered at pH 7.00. Given that a 2- is 4.6 × 10-3 at pH 7.00, what is the final concentration of Ni²+ remaining in solution? Ni2+(aq) + 2 A2(aq) = NIA2(aq) K₁ = 2.00 x 1014

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Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It
forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions.
3
A 27.50 mL sample of 0.0652 M Ni²+ was added to 27.50 mL of 0.195 M iminodiacetic acid (the completely protonated form is
abbreviated as H3A+) buffered at pH 7.00. Given that a A²- is 4.6 × 10-³ at pH 7.00, what is the final concentration of Ni²+
remaining in solution?
Ni²+(aq) + 2 A²¯(aq) = NIA2¯(aq)
Kf = 2.00 × 1014
Transcribed Image Text:Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. It forms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions. 3 A 27.50 mL sample of 0.0652 M Ni²+ was added to 27.50 mL of 0.195 M iminodiacetic acid (the completely protonated form is abbreviated as H3A+) buffered at pH 7.00. Given that a A²- is 4.6 × 10-³ at pH 7.00, what is the final concentration of Ni²+ remaining in solution? Ni²+(aq) + 2 A²¯(aq) = NIA2¯(aq) Kf = 2.00 × 1014
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