Question

To what volume (in mL) would you need

to dilute 35.0 mL of a 1.30 M solution of
KBr to make a 0.0600 M solution of
KBr?

Answer 1

To dilute 35.0 mL of a 1.30 M KBr solution to a 0.0600 M KBr solution, you would need to increase the volume to 754.17 mL using the formula M1V1 = M2V2.

Step-by-step explanation:

To calculate the volume to which you would need to dilute 35.0 mL of a 1.30 M KBr solution to make a 0.0600 M KBr solution, you can use the dilution formula 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 dilute solution. In this case:

• M1 = 1.30 M (initial molarity of KBr)
• V1 = 35.0 mL (initial volume of KBr solution)
• M2 = 0.0600 M (final molarity of KBr desired)
• V2 = ? (final volume of KBr solution needed)

Plugging the values into the equation:

1.30 M × 35.0 mL = 0.0600 M × V2

To find V2, divide both sides by 0.0600 M:

V2 = (1.30 M × 35.0 mL) / 0.0600 M

V2 = 754.17 mL. Therefore, you would need to dilute the solution to 754.17 mL to achieve the desired molarity of 0.0600 M.