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At a certain temperature, silver chloride, AgCl, has a value of Ksp = 5.2 x 10-9. At this temperature, what is the molar solubility of AgCl in the presence of 0.0063 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, lead (i) chloride, PbCl₂, has a value of Ksp = 1.7 x 10-5. At this temperature, what is the molar solubility of PbCl₂ in the presence of 0.45 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, nickel(II) hydroxide, Ni(OH)2, has a value of Kp = 8.2 x 10-16, At this temperature, what is the molar solubility of Ni(OH)2 in a solution buffered at pH 11.33? Report your answer to two significant figures (i.e. 1.2E-8 M). Hint: keep in mind that OH- is a common ion in the dissolution of Ni(OH)2. You can use pH to solve for pOH and [OH-] in this buffered solution. Then use [OH-] to help determine the solubility of the metal hydroxide salt. Answer:

At a certain temperature, silver chloride, AgCl, has a value of Ksp = 5.2 x 10-9. At this temperature, what is the molar solubility of AgCl in the presence of 0.0063 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, lead (i) chloride, PbCl₂, has a value of Ksp = 1.7 x 10-5. At this temperature, what is the molar solubility of PbCl₂ in the presence of 0.45 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, nickel(II) hydroxide, Ni(OH)2, has a value of Kp = 8.2 x 10-16, At this temperature, what is the molar solubility of Ni(OH)2 in a solution buffered at pH 11.33? Report your answer to two significant figures (i.e. 1.2E-8 M). Hint: keep in mind that OH- is a common ion in the dissolution of Ni(OH)2. You can use pH to solve for pOH and [OH-] in this buffered solution. Then use [OH-] to help determine the solubility of the metal hydroxide salt. Answer:

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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At a certain temperature, silver chloride, AgCl, has a value of Ksp = 5.2 x 10-9. At this temperature, what is the molar solubility of AgCl in the presence of 0.0063 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, lead(II) chloride, PbCl₂, has a value of Ksp = 1.7 x 10-5. At this temperature, what is the molar solubility of PbCl₂ in the presence of 0.45 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, nickel(II) hydroxide, Ni(OH)₂, has a value of Kp = 8.2 x 10-16, At this temperature, what is the molar solubility of Ni(OH)₂ in a solution buffered at pH 11.33? Report your answer to two significant figures (i.e. 1.2E-8 M). Hint: keep in mind that OH- is a common ion in the dissolution of Ni(OH)2. You can use pH to solve for pOH and [OH-] in this buffered solution. Then use [OH-] to help determine the solubility of the metal hydroxide salt. Answer:
Transcribed Image Text:At a certain temperature, silver chloride, AgCl, has a value of Ksp = 5.2 x 10-9. At this temperature, what is the molar solubility of AgCl in the presence of 0.0063 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, lead(II) chloride, PbCl₂, has a value of Ksp = 1.7 x 10-5. At this temperature, what is the molar solubility of PbCl₂ in the presence of 0.45 M NaCl ? Report your answer to two significant figures (i.e. 1.2E-3M). Answer: At a certain temperature, nickel(II) hydroxide, Ni(OH)₂, has a value of Kp = 8.2 x 10-16, At this temperature, what is the molar solubility of Ni(OH)₂ in a solution buffered at pH 11.33? Report your answer to two significant figures (i.e. 1.2E-8 M). Hint: keep in mind that OH- is a common ion in the dissolution of Ni(OH)2. You can use pH to solve for pOH and [OH-] in this buffered solution. Then use [OH-] to help determine the solubility of the metal hydroxide salt. Answer:
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