Question

What is the final concentration (m) of a solution prepared by diluting 50.0 ml of a 6.00 m kcl solution to a volume of 1.00 l?

Answer 1

M1V1=M2V2, M - molarity, V- volume, it should be in the same units

So we take 1.00L =1000 mL

6.00*50.0 mL=M2*1000mL

M2=(6.00*50.0 mL)/1000mL=300/1000=0.300 M

Answer 2

Answer: The final concentration of the diluted KCl solution is 0.3 M

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 KCl solution

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

We are given:

Conversion factor:  1 L = 1000 mL

$M_1=6.00M\\V_1=50.0mL\\M_2=?M\\V_2=1.00L=1000mL$

Putting values in above equation, we get:

$6.00\times 50.0=M_2\times 1000\\\\M_2=\frac{6.00\times 50.0}{1000}=0.3M$

Hence, the final concentration of the diluted KCl solution is 0.3 M