O Calculate the number of milliliters of 0.686 M Ba(OH)2 required to precipitate all of the Cu²+ ions in 171 mL of 0.502 M Cul2 solution as Cu(OH)2. The equation for the reaction is: Cul₂ (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + Bal₂ (aq) Volume = mL
O Calculate the number of milliliters of 0.686 M Ba(OH)2 required to precipitate all of the Cu²+ ions in 171 mL of 0.502 M Cul2 solution as Cu(OH)2. The equation for the reaction is: Cul₂ (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + Bal₂ (aq) Volume = mL
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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Please answer both questions
Expert Solution
Step 1
a) given,
CuI2(aq) + Ba(OH)2 -----> Cu(OH)2(s) + BaI2(aq)
For Ba(OH)2 solution:
Concentration of Ba(OH)2 solution = 0.686 M = 0.686 mol/L
Volume of Ba(OH)2 solution = ?
For CuI2 solution:
Concentration of CuI2 solution = 0.502 M = 0.502 mol/L
Volume of CuI2 solution = 171 mL = 0.171 L
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