Traces of heavy metals, such as Cu2+ and Pb2+, in water bodies can be separated through fractional precipitation. A research work investigates the use of NaOH(aq) in separating these two ions in a 1.00 L of water sample that contains 12.70 mg Cu2+ (MM = 63.546 g/mol) and 39.90 mg Pb2+ (MM = 399.32 g/mol) Traces of heavy metals, such as Cu* and Pb", in water bodies can be separated through fractionalprecipitation. A research work investigates the use of NaOH(ag) in separating these two ions in a 1.00 L ofwater sample that cotains 12.70 mg Cu (MM = 63.546 g/mol) and 39.90 mg Pb (MM = 399.32 g/mol).Given:Hydroxide ofCuK2.20 х 10-31.20 x 10 15A. Write the balanced chemical equation and the corresponding Kp expression for the dissolution of thehydroxide salt of (a) Cư* and of (b) Pb** in water.B. Calculate the molar solubility of the hydroxide salt of (a) Cu* and (b) Pb in water. If NaOH(a) isadded gradually to the water sample, which of the two ions is more likely to precipitate first? Explainyour answer.c. Calculate the initial molar concentration of each of the heavy metal ions in the water sample.D. Calculate the equilibrium concentration of NaOH(a) that must be exceeded to initiate the precipitationof the less soluble metal hydroxide.E. How much of the first metal ion is left in the solution when the second ion starts to precipitate? Expressyour answer in percentage (%).

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Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

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

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Chapter11: Solutions

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Traces of heavy metals, such as Cu2+ and Pb2+, in water bodies can be separated through fractional
precipitation. A research work investigates the use of NaOH(aq) in separating these two ions in a 1.00 L of
water sample that contains 12.70 mg Cu2+ (MM = 63.546 g/mol) and 39.90 mg Pb2+ (MM = 399.32 g/mol)

Traces of heavy metals, such as Cu* and Pb", in water bodies can be separated through fractional
precipitation. A research work investigates the use of NaOH(ag) in separating these two ions in a 1.00 L of
water sample that cotains 12.70 mg Cu (MM = 63.546 g/mol) and 39.90 mg Pb (MM = 399.32 g/mol).
Given:
Hydroxide of
Cu
K
2.20 х 10-3
1.20 x 10 15
A. Write the balanced chemical equation and the corresponding Kp expression for the dissolution of the
hydroxide salt of (a) Cư* and of (b) Pb** in water.
B. Calculate the molar solubility of the hydroxide salt of (a) Cu* and (b) Pb in water. If NaOH(a) is
added gradually to the water sample, which of the two ions is more likely to precipitate first? Explain
your answer.
c. Calculate the initial molar concentration of each of the heavy metal ions in the water sample.
D. Calculate the equilibrium concentration of NaOH(a) that must be exceeded to initiate the precipitation
of the less soluble metal hydroxide.
E. How much of the first metal ion is left in the solution when the second ion starts to precipitate? Express
your answer in percentage (%).

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D. Calculate the equilibrium concentration of NaOHa) that must be exceeded to initiate the precipitation
of the less soluble metal hydroxide.
E. How much of the first metal ion is left in the solution when the second ion starts to precipitate? Express
your answer in percentage (%).

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