# Question #457e2

##### 1 Answer

#### Answer:

Here's what I got.

#### Explanation:

**!! LONG ANSWER !!**

All you really need to know here is what it means to **dilute** a solution. If you understand that concept, you don't need to remember any formula.

So, when you're performing a **dilution**, you are essentially doing **one thing**, and that is **increasing the volume** of a solution.

But the thing to remember here is that the **number of moles of solute** is **always kept constant** in a dilution. Always.

In other words, when you're diluting a solution you're adding more *solvent*, while keeping the amount of *solute* constant.

As you know, **molarity** is defined as moles of solute per liter of solution.

#color(blue)("molarity" = "moles of solute"/"liter of solution")#

Notice here that if the number of moles of solute is **kept constant**, increasing the volume of the solution by adding more solvent will **decrease** the concentration, i.e. make the solution *more diluted*.

If you start with a solution that has a molarity of

#color(blue)(overbrace(c_1 xx V_1)^(color(purple)("moles of solute before dilution")) = overbrace(c_2 xx V_2)^(color(purple)("moles of solute after the dilution")))#

That is the formula for **dilution calculations**.

Now, a very useful thing to remember is that the **dilution factor** can be determined by knowing **concentrations** or **volumes of solution**.

#color(blue)("D.F." = V_2/V_1 = c_1/c_2)#

Simply put, to get the dilution factor you either have to know the initial and final concentration of the solution, or the final and initial volume of the solution.

Now let's take a few examples from your list.

**Example 1**

Here you are told that the sample has a volume of *diluent*, which is what you add to dilute the solution, is also equal to

The *diluted volume* is what you get **after** you add the diluent to the sample.

#V_"diluted" = "5 drops" + "5 drops" = "10 drops"#

Now, you know that the initial concentration of the sample is

#"D.F." = (10 color(red)(cancel(color(black)("drops"))))/(5color(red)(cancel(color(black)("drops")))) = 2#

This tells you that you're performing a

#"D.F." = c_1/c_2 implies c_2 = c_1/"D.F." = "10 M"/2 = "5 M"#

**Example 2**

This time, you know the diluted volume and the initial volume of the sample. This means that the volume of diluent was

#V_"diluent" = V_"diluted" - V_"sample"#

#V_"siluent" = "40 drops" - "2 drops" = "38 drops"#

The dilution factor is

#"D.F." = (40color(red)(cancel(color(black)("drops"))))/(2color(red)(cancel(color(black)("drops")))) = 20#

This time, the final concentration will be

#c_2 = c_1/"D.F." = "0.3 M"/20 = "0.015 M"#

**Example 3**

This time, you know the dilution factor and the initial concentration of the sample, which means that you can find its final concentration

#c_2 = c_1/"D.F." = "5 M"/10 = "0.5 M"#

Now you're going to use a bit of algebra to find the volume of the sample and the diluted volume.

If you take the volume of the sample to be

#V_"diluted" = x + "5 mL"#

But since you know the dilution factor, you will have

#"D.F." = ((x + 5)color(red)(cancel(color(black)("mL"))))/(xcolor(red)(cancel(color(black)("mL")))) = 10#

This is equivalent to

#x+5 = 10x implies x = 5/9 = 0.5556#

So, if you start with approximately

Since this is the exact same approach you will need for the other examples, I will leave them to you as practice.