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GarryVolchara [31]
2 years ago
14

An unknown aqueous metal analysis yielded a detector response of 0.255. When 1.00 mL of a solution containing 100.0 ppm of the m

etal was mixed with 99.0 mL of the unknown, the detector signal increased to 0.502. Calculate the concentration of the metal in the unknown solution. Report your answer in ppm
Chemistry
1 answer:
AVprozaik [17]2 years ago
3 0

Answer:

1.022ppm is the unknown concentration of the metal

Explanation:

Based on Lambert-Beer law, the increasing in signal of a detector is directly proportional to its concentration.

The unknown concentration (X) produces a signal of 0.255

99mL * X + 1mL * 100ppm / 100mL produces a signal of 0.502

0.99X + 1ppm produce 0.502, thus, X is:

0.255 * (0.99X + 1 / 0.502) =

X = 0.503X + 0.508

0.497X = 0.508

X =

1.022ppm is the unknown concentration of the metal

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What are the uses of solution?<br>​
Ilia_Sergeevich [38]

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Explanation:

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Answer : The correct options are, SnO_2+2H_2\rightarrow Sn+2H_2O and 2Al+6HCl\rightarrow 2AlCl_3+3H_2

Explanation :

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Hence, the options B and E are single displacement reactions.

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