Question: Calculate the actual concentration of Cu2+ ion in your samples. Becaus

Question

Question:

Calculate the actual concentration of Cu2+ ion in your samples. Because you are simply diluting a copper-containing solution of known concentration, you can use the equation:

(conc. of original solution )*(volume of standard Cu2+) = (concentration of dilute solution)*(total solution volume)

Lab Notes:

Cuvette #1:

4mL 0.06 M copper (II) sulfate

6mL 1.0 M nitric acid (HNO3)

[Cu^2+] = 0.024 M

absorbance: 0.25

Cuvette #2:

7mL 0.06 M copper (II) sulfate

3mL 1.0 M nitric acid (HNO3)

[Cu^2+] = 0.042 M

absorbance: 0.44

Cuvette #3:

10mL 0.06 M copper (II) sulfate

0mL 1.0 M nitric acid (HNO3)

[Cu^2+] = 0.06M

absorbance: 0.63

Explanation / Answer

Hi! Welcome to Chegg

Cuvette #1

(4 mL)(0.06 M) / (6+4) mL = 0.024 M

Cuvette #2

(7 mL)(0.06 M) / (7+3) mL = 0.042 M

Cuvette #3

(10 mL)(0.06 M) / (10+0) mL = 0.06 M

Related Questions

Navigate

• Browse (All)
• Browse Q
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.