How much water must be added 6.0 M silver nitrate in order to make 500 mL of 1.2 M solution?

Answer 1

To calculate the amount of water needed to dilute the 6.0 M silver nitrate to 1.2 M, we can use the formula for dilution:

M1V1 = M2V2

Where:
M1 = initial molarity (6.0 M)
V1 = volume of the initial solution (unknown)
M2 = final molarity (1.2 M)
V2 = total volume of the final solution (500 mL)

Plugging in the values:

6.0 M * V1 = 1.2 M * 500 mL

V1 = (1.2 M * 500 mL) / 6.0 M
V1 = 100 mL

This means that you have 100 mL of the 6.0 M silver nitrate solution. To make a 1.2 M solution, you need to add water to bring the total volume to 500 mL.

Amount of water to be added = 500 mL - 100 mL = 400 mL

Therefore, 400 mL of water must be added to 100 mL of 6.0 M silver nitrate to make a 500 mL solution with a concentration of 1.2 M.