A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O4 at 25 °C (solution A, oxalate ion = C₂O4²- ). 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)
A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O4 at 25 °C (solution A, oxalate ion = C₂O4²- ). 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)
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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![### Problem Statement:
A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O₄ at 25 °C (solution A, oxalate ion = C₂O₄²⁻). 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 × 10⁻⁹ at 25 °C?
### Instructions:
Enter your answer with two **significant figures**, without units, and in millimolarity (mM) where:
\[ \text{millimolarity} = (\text{molarity})(1000) \]
### Possible Answers:
- 0.001 (with margin: 0)
- 0.0011 (with margin: 0)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc788d0c0-fee4-4de6-a09a-88d5a7462434%2Fe4627921-cf02-46b1-bb98-9fbf96adafd2%2F6xs2cvq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem Statement:
A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O₄ at 25 °C (solution A, oxalate ion = C₂O₄²⁻). 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 × 10⁻⁹ at 25 °C?
### Instructions:
Enter your answer with two **significant figures**, without units, and in millimolarity (mM) where:
\[ \text{millimolarity} = (\text{molarity})(1000) \]
### Possible Answers:
- 0.001 (with margin: 0)
- 0.0011 (with margin: 0)
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