Final answer:
Approximately 167.31 mL of water needs to be added to 25 mL of a 0.250 M Br solution to produce a diluted solution of 0.0325 M concentration.
Step-by-step explanation:
To determine the volume of water that must be added to 25 ml of a 0.250 M Br solution to get a 0.0325 M solution, we can use the dilution equation M1V1 = M2V2, where M1 and V1 are the molarity and volume of the concentrated solution, and M2 and V2 are the molarity and volume of the diluted solution, respectively.
First, let's identify our variables:
- M1 = 0.250 M (initial molarity)
- V1 = 25 mL (initial volume)
- M2 = 0.0325 M (final molarity)
- V2 = ? (final volume to find)
By substituting the known values into the dilution equation, we get:
0.250 M × 25 mL = 0.0325 M × V2
Now, solve for V2:
V2 = (0.250 M × 25 mL) / 0.0325 M
V2 = 192.3077 mL
Thus, the final volume is approximately 192.31 mL. To find the volume of water that needs to be added, subtract the initial volume from the final volume:
Volume of water added = V2 - V1 = 192.31 mL - 25 mL = 167.31 mL
167.31 mL of water needs to be added to the 25 ml of a 0.250 M Br solution to produce a 0.0325 M solution.