Question

A 58.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 193 mL of water. What is the final concentration? Assume the volumes are additive.

Name: A 58.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 193 mL of water. What is the final concentration? Assume the volumes are additive.
Uploaded: 2023-07-09T09:54:56-08:00
Duration: 1 min 22 s
Channel: Adi S
Description: A 58.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 193 mL of water. What is the final concentration? Assume the volumes are additive.

          A 58.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 193 mL of water. What is the final concentration? Assume the volumes are additive.

A 58.0 mL aliquot of a 1.50 M solution is diluted to a total volume of 238 mL. A 119 mL portion of that solution is diluted by adding 193 mL of water. What is the final concentration? Assume the volumes are additive.

Added by Steven M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

07/09/2023

Step 1

Using the dilution formula: \[ C_1V_1 = C_2V_2 \] Where: - \( C_1 \) is the initial concentration = 1.50 M - \( V_1 \) is the initial volume = 58.0 mL - \( V_2 \) is the final volume = 238 mL Solving for \( C_2 \): \[ C_2 = \frac{C_1V_1}{V_2} = \frac{1.50 Show more…

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