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4. If you use 25.0 mL of the Calcium Chloride solution and an excess of Sodium Carbonate, how many grams of Calcium Carbonate should be theoretically be produced?

4. If you use 25.0 mL of the Calcium Chloride solution and an excess of Sodium Carbonate, how many grams of Calcium Carbonate should be theoretically be produced?

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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Please help with question 4
ice Chem 105 UHI Safety: While these are household items that you could easily purchase at the store, please understand that this is still for chemistry purposes. Do not INGEST anything or leave readily available for pets and young children to get into (especially your chalk, um-I mean your final precipitate). All items can be thrown away at the end. Ice melt solutions can be thrown away outside away from pet areas. Even though Calcium Carbonate is relatively harmless-please note that this should not be ingested. Prelab: 1. If you had to make a 0.750M solution of Na₂CO3 from 100mL of solution, determine the mass of Sodium Carbonate necessary. 1000 ML/LX, 750 m04/L = .075 mol mass of Na₂CO3 = 1069/molx .075md=7.95g Na2CO3-1069/mol 2. If you had to make a 0.250M solution of CaCl₂ from 100mL of solution, determine the mass of Calcium Chloride necessary. 250m 1000 me X100ML = ·025ML of 3. If you use 10.0 mL of the Sodium Carbonate solution and an excess of Calcium Chloride, how many grams of Calcium Carbonate should be theoretically be produced? 10.0mL Mograms Na203 +CaC12 > CaCO3+ 2NaC/ .750M 4. If you use 25.0 mL of the Calcium Chloride solution and an excess of Sodium Carbonate, how many grams of Calcium Carbonate should be theoretically be produced? 5. Using the information in problems 3 and 4, what is the theoretical yield of 25.0mL of a 0.250M solution of CaCl₂ when mixed with 10.0 mL of a 0.750M Sodium Carbonate solution? 6. Suppose the student performs the experiment in the previous problem, what is the percent yield if they generate 0.565g of CaCO3?
Transcribed Image Text:ice Chem 105 UHI Safety: While these are household items that you could easily purchase at the store, please understand that this is still for chemistry purposes. Do not INGEST anything or leave readily available for pets and young children to get into (especially your chalk, um-I mean your final precipitate). All items can be thrown away at the end. Ice melt solutions can be thrown away outside away from pet areas. Even though Calcium Carbonate is relatively harmless-please note that this should not be ingested. Prelab: 1. If you had to make a 0.750M solution of Na₂CO3 from 100mL of solution, determine the mass of Sodium Carbonate necessary. 1000 ML/LX, 750 m04/L = .075 mol mass of Na₂CO3 = 1069/molx .075md=7.95g Na2CO3-1069/mol 2. If you had to make a 0.250M solution of CaCl₂ from 100mL of solution, determine the mass of Calcium Chloride necessary. 250m 1000 me X100ML = ·025ML of 3. If you use 10.0 mL of the Sodium Carbonate solution and an excess of Calcium Chloride, how many grams of Calcium Carbonate should be theoretically be produced? 10.0mL Mograms Na203 +CaC12 > CaCO3+ 2NaC/ .750M 4. If you use 25.0 mL of the Calcium Chloride solution and an excess of Sodium Carbonate, how many grams of Calcium Carbonate should be theoretically be produced? 5. Using the information in problems 3 and 4, what is the theoretical yield of 25.0mL of a 0.250M solution of CaCl₂ when mixed with 10.0 mL of a 0.750M Sodium Carbonate solution? 6. Suppose the student performs the experiment in the previous problem, what is the percent yield if they generate 0.565g of CaCO3?
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