A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O4 at 25 °C (solution A, oxalate ion = C₂04²-). Anaqueous solution of Ca(NO3)2 with a volume of 50.0 mL (solution B) is added to solution A, at thesame temperature.Above what minimum concentration must Ca(NO3)2 in solution B be, prior to mixing, to causeCaC₂O4 to precipitate given that for CaC₂O4, Ksp = 2.7 x 10-⁹ at 25 °C?Enter your answer with two significant figures, without units, and in millimolarity (mM) where:millimolarity = (molarity)(1000)

Answered: A chemist has a 50.0 mL sample of 0.010…

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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A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O4 at 25 °C (solution A, oxalate ion = C₂04²-). An
aqueous solution of Ca(NO3)2 with a volume of 50.0 mL (solution B) is added to solution A, at the
same temperature.
Above what minimum concentration must Ca(NO3)2 in solution B be, prior to mixing, to cause
CaC₂O4 to precipitate given that for CaC₂O4, Ksp = 2.7 x 10-⁹ at 25 °C?
Enter your answer with two significant figures, without units, and in millimolarity (mM) where:
millimolarity = (molarity)(1000)

Expert Solution

Step 1: Solubility product

In this chemical scenario, we are exploring a common concept in chemistry: the solubility of ionic compounds and the effects of adding solutions with common ions. The goal is to determine the minimum concentration of Ca²⁺ ions in an aqueous solution of Ca(NO₃)₂ (solution B) needed to cause the precipitation of CaC₂O₄ from a separate solution containing oxalate ions, Na₂C₂O₄ (solution A).

Solubility product constants (Ksp) play a key role in predicting whether a precipitate will form when two solutions are mixed. In this case, we're given the Ksp value for CaC₂O₄, which is the solubility product constant for the dissolution of calcium oxalate in water. When the product of the concentrations of Ca²⁺ and C₂O₄^2- ions exceed this constant, precipitation occurs.

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