Question

A chemist dilutes a 1.0 mL sample of 2.0 M KNO3 by adding water to it. If the concentration of the solution that is obtained is 0.0080 M, what is its volume? Use mc016-1.jpg.

Answer 1

250 ml.  Use the equation 

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

So:

(2 M) x (1ml) = (.008 M) x (X ml)

X = 250 ml

Answer 2

Answer: The volume of the diluted solution is 250 mL.

Explanation:

To calculate the molarity of the diluted solution, we use the equation:

$M_1V_1=M_2V_2$

where,  

$M_1\text{ and }V_1$ are the molarity and volume of the concentrated $KNO_3$ solution

$M_2\text{ and }V_2$ are the molarity and volume of diluted $KNO_3$ solution

We are given:

$M_1=2M\\V_1=1mL\\M_2=0.008M\\V_2=?mL$  

Putting values in above equation, we get:  

$2\times 1=0.008\times V_2\\\\V_2=250mL$

Hence, the volume of the diluted solution is 250 mL.