3. 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). Given: Hydroxide of Ksp Cu²* 2.20 x 10-20 Pb2+ 1.20 × 10-15 A. Write the balanced chemical equation and the corresponding Ksp expression for the dissolution of the hydroxide salt of (a) Cu²* and of (b) Pb²* in water. B. Calculate the molar solubility of the hydroxide salt of (a) Cu²* and (b) Pb²* in water. If NaOH(aq) 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(aq) 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 (%).
3. 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). Given: Hydroxide of Ksp Cu²* 2.20 x 10-20 Pb2+ 1.20 × 10-15 A. Write the balanced chemical equation and the corresponding Ksp expression for the dissolution of the hydroxide salt of (a) Cu²* and of (b) Pb²* in water. B. Calculate the molar solubility of the hydroxide salt of (a) Cu²* and (b) Pb²* in water. If NaOH(aq) 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(aq) 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 (%).
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter7: Chemical Reactions: An Introduction
Section: Chapter Questions
Problem 10A
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Answer C, D and E only
Transcribed Image Text:3. 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).
Given:
Hydroxide of
Ksp
Cu2+
2.20 × 10-20
Pb2+
1.20 x 10-15
A. Write the balanced chemical equation and the corresponding Ksp expression for the dissolution of the
hydroxide salt of (a) Cu²* and of (b) Pb²* in water.
B. Calculate the molar solubility of the hydroxide salt of (a) Cu²* and (b) Pb²* in water. If NaOH(aq) 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(aq) 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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