Answer :

To prepare a 2.00 M [tex]NH_3[/tex] solution in 2.00 L, you would need 250 ml of the 16 M [tex]NH_3[/tex] solution.

To determine how many milliliters (ml) of a 16 M [tex]NH_3[/tex] solution are needed to prepare a 2.00 L solution with a concentration of 2.00 M, we can use the concept of molarity, which is the amount of solute (in moles) divided by the volume of the solution (in liters).

First, we need to calculate the amount of [tex]NH_3[/tex] required to achieve a concentration of 2.00 M in a 2.00 L solution. The formula for molarity is:

Molarity = moles of solute/volume of solution (in liters)

2.00 M = moles of [tex]NH_3[/tex] / 2.00 L

Rearranging the equation, we have:

moles of [tex]NH_3[/tex] = 2.00 M × 2.00 L = 4.00 moles

Now, we can use the given concentration of the 16 M [tex]NH_3[/tex] solution to calculate the volume of the solution needed.

Molarity = moles of solute/volume of solution (in liters)

16 M = 4.00 moles/volume of 16 M [tex]NH_3[/tex] (in liters)

Rearranging the equation, we have:

volume of 16 M [tex]NH_3[/tex] = 4.00 moles / 16 M = 0.25 L

Finally, we need to convert the volume from liters to milliliters:

0.25 L × 1000 ml/L = 250 ml

To learn more about molarity

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