Question

(c) How many mL of the 0.15 M solution should be diluted to prepare 125.0 mL of a 0.050 M solution?

Answer 1

To prepare a 0.050 M solution from a 0.15 M solution, 41.67 mL of the 0.15 M solution should be diluted.

Step-by-step explanation:

To find out how many mL of the 0.15 M solution should be diluted to prepare 125.0 mL of a 0.050 M solution, we can use the equation:

(initial concentration)(initial volume) = (final concentration)(final volume)

Plugging in the values, we get:

(0.15 M)(x mL) = (0.050 M)(125.0 mL)

Solving for x, we find that x = (0.050 M)(125.0 mL) / (0.15 M). Therefore, x = 41.67 mL.

Answer 2

41 ml of the 0.15 solution should be diluted with 84 ml of water to prepare 125.0 ml of a 0.050 M solution

Step-by-step explanation:

since the final solution has 0.050M , the amount of moles that should be present in 125 ml are

amount of moles = molarity * volume

amount of moles = 0.050 moles/L * 0.125L = 6.25*10⁻³ moles

therefore for a solution 0.15 M

amount of moles = molarity * volume

6.25*10⁻³ moles = 0.15 M*volume

volume = 0.041 L = 41 ml

if the number of moles are contained in 41 ml , the rest should be solvent ( water)

amount of water to dilute = 125 ml - 41 ml = 84 ml

then we will have 6.25*10⁻³ moles in 125 ml