2. Use the method from 1. above to calculate the volumes needed to prepare 5 CV* solutions, each at 3.0 mL, that span the range from 0 to 1.0 x 105 M CV*. Use the table below as a guide. Copy this table into your notebook to use in the lab. Solution 1 2 3 45 4 [CV] (M) 0.0 Vol. of 2.0 x 105 M CV* (ml) 0.0 Vol. of H₂O (mL) 3.0
2. Use the method from 1. above to calculate the volumes needed to prepare 5 CV* solutions, each at 3.0 mL, that span the range from 0 to 1.0 x 105 M CV*. Use the table below as a guide. Copy this table into your notebook to use in the lab. Solution 1 2 3 45 4 [CV] (M) 0.0 Vol. of 2.0 x 105 M CV* (ml) 0.0 Vol. of H₂O (mL) 3.0
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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Solve number 2. I gave the answer too number 1 to help solve 2
![0:49 PM Sat Feb 4
T
1. In this experiment, you will make a set of solutions containing different concentrations of
crystal violet (CV) by mixing different volumes of a stock CV* solution with water to give final
volumes of 3.0 mL. The stock solution of CV* has a concentration of 2.0 x 10-5 M and is dark
purple. The diluted solutions will be prepared in cuvettes.
2.0 x 105 M CV+
(purple)
H₂O
V₁
Solution
1
2
3
4
5
[CV] (M)
0.0
0}
diluted samples of CV*
in cuvettes
Vol of Stock Solh = 1.125mL
Vol of water = 1.875m
Use c₁V₁= C₂V₂ to calculate the volume of the stock 2.0 x 105 M CV AND the volume of water to
make a 3.0 mL sample of 7.5 x 10-6 M CV+. Show all of your calculations.
2.0 x 105 x V₁ = 7.5x10-6 * 3
V₁ = 1.125mL
3.0 mL= V₂
Vol. of 2.0 x 105 M CV+ (ml)
0.0
2. Use the method from 1. above to calculate the volumes needed to prepare 5 CV* solutions,
each at 3.0 mL, that span the range from 0 to 1.0 x 105 M CV. Use the table below as a guide.
Copy this table into your notebook to use in the lab.
☎ @ 80%
+ :
Vol. of H₂O (mL)
3.0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5d95d0cb-9ec4-45a1-97ed-91d8eea226dd%2Ff903eb92-26ff-4a5a-b4e6-1902da159556%2Fm9gd5x9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:0:49 PM Sat Feb 4
T
1. In this experiment, you will make a set of solutions containing different concentrations of
crystal violet (CV) by mixing different volumes of a stock CV* solution with water to give final
volumes of 3.0 mL. The stock solution of CV* has a concentration of 2.0 x 10-5 M and is dark
purple. The diluted solutions will be prepared in cuvettes.
2.0 x 105 M CV+
(purple)
H₂O
V₁
Solution
1
2
3
4
5
[CV] (M)
0.0
0}
diluted samples of CV*
in cuvettes
Vol of Stock Solh = 1.125mL
Vol of water = 1.875m
Use c₁V₁= C₂V₂ to calculate the volume of the stock 2.0 x 105 M CV AND the volume of water to
make a 3.0 mL sample of 7.5 x 10-6 M CV+. Show all of your calculations.
2.0 x 105 x V₁ = 7.5x10-6 * 3
V₁ = 1.125mL
3.0 mL= V₂
Vol. of 2.0 x 105 M CV+ (ml)
0.0
2. Use the method from 1. above to calculate the volumes needed to prepare 5 CV* solutions,
each at 3.0 mL, that span the range from 0 to 1.0 x 105 M CV. Use the table below as a guide.
Copy this table into your notebook to use in the lab.
☎ @ 80%
+ :
Vol. of H₂O (mL)
3.0
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