Iminodiacetic acid (IDA) is often used in ion exchange resins as a way to remove heavy metals from industrial waste waters. Itforms a 2:1 complex with many heavy metals, with a high selectivity for divalent over monovalent ions.A 22.50 mL sample of 0.0454 M Ni²+ was added to 22.50 mL of 0.190 M iminodiacetic acid (the completely protonated form isabbreviated as H, A*) buffered at pH 7.00. Given that ais 4.6 x 10-3 at pH 7.00, what is the final concentration of Ni²+remaining in solution?Ni²+ (aq) + 2 A² (aq) = N₁A3(aq)[Ni²+] =K₁ = 2.00 × 10¹4M

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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. A 22.50 mL sample of 0.0454 M Ni2+ was added to 22.50 mL of 0.190 M iminodiacetic acid (the completely protonated form is abbreviated as H, A*) buffered at pH 7.00. Given that ais 4.6 x 10-3 at pH 7.00, what is the final concentration of Ni²+ remaining in solution? Ni²+ (aq) + 2 A²-(aq) = NiA² (aq) [Ni²+] = K₁ = 2.00 × 10¹4 M

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 22.50 mL sample of 0.0454 M Ni2+ was added to 22.50 mL of 0.190 M iminodiacetic acid (the completely protonated form is abbreviated as H, A*) buffered at pH 7.00. Given that ais 4.6 x 10-3 at pH 7.00, what is the final concentration of Ni²+ remaining in solution? Ni²+ (aq) + 2 A²-(aq) = NiA² (aq) [Ni²+] = K₁ = 2.00 × 10¹4 M

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 26P

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