Help asap please. A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered and dried and then found to have a mass of 217 mg. What mass of barium was in the original solution? (Assume that all of the barium was precipitated out of solution by the reaction.)

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Ответ:

divagothboi

10.05.2020

Chemistry

15.3 s

Explanation:

Let's consider the first-order decomposition of a generic compound A. We can find the concentration at a certain time using the following expression.

$[A]_{t}=[A]_{0}.e^{-k\times t }$

where,

$[A]_{t}$ : concentration of A at a time t

$[A]_{0}$ : initial concentration of A

k: rate constant

When 75% of A decomposes, the remaining concentration is 25% ( $[A]_{t}$ = 0.25 $[A]_{0}$ ). The required time is:

$[A]_{t}/[A]_{0}=e^{-0.0909s^{-1} \times t }\\$

$0.25[A]_{0}/[A]_{0}=e^{-0.0909s^{-1} \times t }\\$

t = 15.3 s

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