Answer:
The concentration of the original solution is 1x10*-4 M
Explanation:
[Fe3+} = 2.50 x 10−5 M
It means that in 1 L, I have 2,50 x 10−5 moles of cation.
These are the rules of three involved.
1 L ______ 2,50 x 10−5 moles
0,1 L _____ (0,1 L . 2,50 x 10−5 m) / 1L = 2,50 x 10−6 moles
As the total volume of solution is 100 ml, the 2,50 x 10−6 moles are also in 25 ml of the stock solution.
So:
0,025 L _____ 2,50 x 10−6 moles
1 L _________ (1L . 2,50 x 10−6 m) / 0,025 L = 1x10*-4 M
A student in the lab prepared a cereal sample solution for spectroscopic analysis as described in the lab manual, and found the concentration of Fe3+ in the sample to be 2.50 x 10−5 M. The concentration of the original solution is 1.00 × 10⁻⁴ M.
The concentration of a solution is the estimate of how much solute has been dissolved in the solvent.
The molar concentration of Fe3+ = 2.50 × 10⁻⁵ M
∴
In 1 liter, there are 2.50 × 10⁻⁵ M of Fe3+
Now in 100 mL which is equivalent to 0.1 L, the concentration of Fe3+ will be:
[tex]\mathbf{= \dfrac{0.1 \ L \times 2.50 \times 10^{-5} \ M }{1 \ L}}[/tex]
= 2.5 × 10⁻⁶ M
Since the total volume of the solution is 100 mL, the 2.5 × 10⁻⁵ M is also present in 25 mL of the stock(original) solution.
∴
[tex]\mathbf{= \dfrac{1 \ liter \times 2.5 \times 10^{-6} \ M}{0.025 \ L}}[/tex]
= 1.00 × 10⁻⁴ M concentration of the original solution
Therefore, we can conclude that the concentration of the original solution is 1.00 × 10⁻⁴ M.
Learn more about the concentration of a solution here:
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