Please help with question 4 iceChem 105 UHISafety:While these are household items that you could easily purchase at the store, please understandthat this is still for chemistry purposes. Do not INGEST anything or leave readily available for petsand young children to get into (especially your chalk, um-I mean your final precipitate). Allitems can be thrown away at the end. Ice melt solutions can be thrown away outside awayfrom pet areas. Even though Calcium Carbonate is relatively harmless-please note that thisshould not be ingested.Prelab:1. If you had to make a 0.750M solution of Na₂CO3 from 100mL of solution, determine themass of Sodium Carbonate necessary.1000 ML/LX, 750 m04/L = .075 molmass of Na₂CO3 = 1069/molx .075md=7.95gNa2CO3-1069/mol2. If you had to make a 0.250M solution of CaCl₂ from 100mL of solution, determine themass of Calcium Chloride necessary.250m1000 meX100ML =·025ML of3. 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/.750M4. 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 a0.250M solution of CaCl₂ when mixed with 10.0 mL of a 0.750M Sodium Carbonatesolution?6. Suppose the student performs the experiment in the previous problem, what is thepercent yield if they generate 0.565g of CaCO3?

Answered: Image /qna-images/answer/4d5207d5-9065-4f30-8b7e-40067f8d563a.jpg

Answered: 4. If you use 25.0 mL of the Calcium…

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

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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Question

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?

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