1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain?Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 3 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction? 5)What is the maximum mass (in grams) of CaCO3 that could form in the precipitation reaction described in Question 4?Include the correct number of significant figures in your answer.

The chemical reaction between CaCl2 and Na2CO3 is CaCl2(aq) + Na2CO3(aq)---->2NaCl(aq) +…

Answered: 1)What is the theoretical yield (in…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

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1)What is the theoretical yield (in grams) of CaCO₃ in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl₂ in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na₂CO₃ in 30 mL of water?
Include the appropriate number of significant figures in your answer.

2)Suppose that 0.814 g of CaCO₃ is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?
Report your answer to the correct number of significant figures.

3)A solution of Na₂CO₃ is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na₂CO₃ does this solution contain?

Express your answer to the correct number of significant figures.

4)Suppose the Na₂CO₃ solution described in Question 3 is added to a solution that contains excess CaCl₂? What is the maximum number of moles of solid CaCO₃ that can form in the resulting precipitation reaction?

5)What is the maximum mass (in grams) of CaCO₃ that could form in the precipitation reaction described in Question 4?
Include the correct number of significant figures in your answer.

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