Question

A 47.71 mL sample of a 0.200 M solution of barium nitrate is mixed with 16.41 mL of a 0.250 M solution of potassium sulfate. Assuming that all ionic species are completely dissociated and the temperature is 25°C, what is the osmotic pressure of the mixture in torr?

Name: A 47.71 mL sample of a 0.200 M solution of barium nitrate is mixed with 16.41 mL of a 0.250 M solution of potassium sulfate. Assuming that all ionic species are completely dissociated and the temperature is 25°C, what is the osmotic pressure of the mixture in torr?
Uploaded: 2022-06-22T07:20:30-08:00
Duration: 2 min 50 s
Channel: Madhur L
Description: A 47.71 mL sample of a 0.200 M solution of barium nitrate is mixed with 16.41 mL of a 0.250 M solution of potassium sulfate. Assuming that all ionic species are completely dissociated and the temperature is 25°C, what is the osmotic pressure of the mixture in torr?

          A 47.71 mL sample of a 0.200 M solution of barium nitrate is mixed with 16.41 mL of a 0.250 M solution of potassium sulfate. Assuming that all ionic species are completely dissociated and the temperature is 25°C, what is the osmotic pressure of the mixture in torr?

A 47.71 mL sample of a 0.200 M solution of barium nitrate is mixed with 16.41 mL of a 0.250 M solution of potassium sulfate. Assuming that all ionic species are completely dissociated and the temperature is 25°C, what is the osmotic pressure of the mixture in torr?

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Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

06/22/2022

Step 1

Given: - Moles of barium nitrate = 9.5 x 10^-3 moles - Moles of potassium sulfate = 4.10 x 10^-3 moles Total moles = 9.5 x 10^-3 + 4.10 x 10^-3 = 0.0136 moles Show more…

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A 47.71 mL sample of a 0.200 M solution of barium nitrate is mixed with 16.41 mL of a 0.250 M solution of potassium sulfate. Assuming that all ionic species are completely dissociated and the temperature is 25°C, what is the osmotic pressure of the mixture in torr?