The wastewater solution from a factory containing high levels of salts needs to be diluted before it can be released into the environment. Therefore, two containers of waste solution are separated by a semipermeable membrane and pressure is applied to one container, forcing only water molecules through the membrane and diluting the waste solution in the other container. As dilution continues, higher and higher pressures are needed to counteract the natural tendency for the water molecules to have a net flow back toward the more concentrated solution. What was the applied pressure at the end of this process if the final concentrations of the solutions were 0.053 M and 0.170 M at a temperature of 23 ∘C?

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Chemistry

28 June, 11:06

The wastewater solution from a factory containing high levels of salts needs to be diluted before it can be released into the environment. Therefore, two containers of waste solution are separated by a semipermeable membrane and pressure is applied to one container, forcing only water molecules through the membrane and diluting the waste solution in the other container. As dilution continues, higher and higher pressures are needed to counteract the natural tendency for the water molecules to have a net flow back toward the more concentrated solution. What was the applied pressure at the end of this process if the final concentrations of the solutions were 0.053 M and 0.170 M at a temperature of 23 ∘C?

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Joel Padilla · Answer 1

The applied pressure at the end of this process is P = - 2.859atm

Explanation:

Write down the given values

there are concentration of two solutions

S1 = 0.053 M

S2 = 0.170 M

Temperature (T) = 23°C

that is written as 298 K

it can be solved by multiplying ans subtracting the values

P=MR1-MR2

0.053 M * 0.082 * 298 - 0.170 M * 0.082 * 298

= 1.295 - 4.15412

P = - 2.859atm