Question

A laboratory experiment requires 4.8 l of a 2.5 m solution of sulfuric acid (h2so4), but the only available h2so4 is a 6.0 m stock solution. how could you prepare the solution needed for the lab experiment?

Answer 1

To determine the amount of 6.0 M H2SO4 needed for the preparation, equate the number of moles of the 6.0 M and 2.5 M H2SO4 solution. This is done as follows
 
                                             M1 x V1 = M2 x V2

Substituting the known variables,
 
                                             (6.0 M) x V1 = (2.5 M) x (4.8 L)

Solving for V1 gives an answer of V1 = 2 L. Thus, to prepare the needed solution, dilute 2 L of 6.0 M H2SO4 solution with water until the volume reach 4.8 L. 

Answer 2

Answer:

We will take 2 L of sulfuric acid stock solution, and then will add 4L to it.

Explanation:

Given:

Concentration of stock solution = 6 M

volume of stock required = to be calculated =?

Concentration of required solution = 2.5 M

Volume of required solution = 4.8 L

This problem is based on dilution.

We will take some volume of sulfuric acid and will dilute it to 4.8 L.

Now in order to calculate the volume of sulfuric acid required we will use following formula.

M₁V₁=M₂V₂

M₁= molarity of stock solution = 6 M

V₁ = volume of stock solution = ?

M₂ =molarity of required solution = 2.5 M

V₂ = volume of required solution = 4.8 L

Putting values,

$V_{1}=\frac{M_{2}V_{2}  }{M_{1} }$

$V_{1}=\frac{2.5X4.8}{6}=2L$

Thus we will take 2 L of sulfuric acid stock solution, and then will add 4L to it.