# Question #a3b28

##### 1 Answer

#### Answer:

#### Explanation:

I'll stat with a quick rundown of what *dilution* something actually means.

As you know, the **molarity** of a solution tells you how many *moles of solute* you get **per liter** of solution.

In simple terms, molarity is a measure of how concentrated a solution is in terms of the *amount of solute* it contains per liter of solution.

When your aim is to **dilute a solution**, you're essentially keeping the amount of solute **constant** while **increasing** the volume of the solution.

This can be written as

#color(blue)( overbrace(c_1 xx V_1)^(color(purple)("moles of solute in initial solution")) = overbrace(c_2 xx V_2)^(color(purple)("moles of solute in target solution")))#

Here

Notice that you can rewrite this equation as

#c_1/c_2 = V_2/V_1#

The ratio between the volume of the *target solution* and the volume of the *initial solution* gives you the **dilution factor**.

#color(blue)("D.F". = V_"final"/V_"initial")#

For example, in order to perform a

#c_2 = 1/2 * c_1#

will give you

#V_2/V_1 = (color(red)(cancel(color(black)(c_1))))/(1/2 * color(red)(cancel(color(black)(c_1)))) = 2#

Notice that you don't need concentration values to find the dilution factor of a solution, as is the case with your example.

In your case, you want to perform a

#"D.F." = 64 = V_2/V_1#

This tells you that the volume of the target solution must be

#64 = V_2/V_1 implies V_2 = 64 * V_1#

Plug in your value for the volume of the aliquot to get

#V_2 = 64 * "1.194 mL" = "76.416 mL"#

Since the volume of the target solution will be equal to

#V_2 = V_1 + V_"saline"#

it follows that you will need to add

#V_"saline" = "76.416 mL" - "1.194 mL" = color(green)(color(green)("75.22 mL")#

of sterile saline solution to your anti-cancer drug to perform a