If the absorbance of a solution of copper(II) ion decreases by 28.00% upon dilution, what volume of water was added to 20.0 mL of a 1.20 M solution of Cu2+(aq)?
Absorbance and concentrations are linearly related. That is
A = e*l*c
Where A is absorbance
l is path length
c is concentration
e = molar absorptivity
Here:
A2 = (100-28)% of A1
= 72 % of A1
So,
A2/A1 = 0.72
So,
A2/A1 = C2/C1
0.72 = C2/1.20
C2 = 0.864 M
use dilution formula
M1*V1 = M2*V2
1---> is for stock solution
2---> is for diluted solution
Given:
M1 = 1.2 M
M2 = 0.864 M
V1 = 20 mL
use:
M1*V1 = M2*V2
V2 = (M1 * V1) / M2
V2 = (1.2*20)/0.864
V2 = 27.8 mL
volume of water added = V2 - V1
= 27.8 mL - 20.0 mL
= 7.8 mL
Answer: 7.8 mL
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