Answer:
concentration of diluted solution = 0.0125 ( ± 0.0002)M
Uncertainty = ± 0.0002
Explanation:
Given that
Initial volume of Cu2+ = 4.00 (±0.01) mL
Initial molarity 0f Cu2+ = 0.302 (±0.004) M
transferred to 100.00 (±0.08) Class A volumetric flask
first we get amount of water added
100.00 (±0.08) - 4.00 (±0.01) = 96 ± (0.09)
Now according to law of dilution
The concentration of Cu2+ after adding water
M1V1 = M2V2
we substitute
0.302 (±0.004) * 4.00 (±0.01) = x * 96 ± (0.09)
Now the multiplication of two digits with uncertainty is
(0.004/0.302) * 100 = 1.32% ; (0.01/4.00) * 100 = 0.25%
= [0.302 ( ± 1.32% )] * [ 4.00 ± (0.25%)]
= 1.208 ±(1.57%)
1.57/100 * 1.208 = 0.0189
so
= (1.208 ± 0.0189)
now substitute in our previous equation
1.208 ± (0.0189) = x * 96 ± (0.09)
x = 1.208 ± (0.0189) / 96 ± (0.09)
{ 0.09/96 * 100 = 0.094% }
so x = 1.208 ± (1.57%) / 96 ± (0.094% )
x = 0.0125 ± ( 1.664)
now( 1.664/100 * 0.0125)
= ± 0.000208
Hence
concentration of diluted solution = 0.0125 ( ± 0.0002)M
Uncertainty = ± 0.0002
