Alaboratory 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? show all the work used to find your answer.

Take 2.0 L of the H2SO4 stock solution of 6.0 M and dilute it to 4.8 L

Explanation:

For The exercise we are going to need the next equation:

(Final concentration)(final volume) = (initial concentration)(initial volume) or CfVf=CiVi

The final solution is the one required to the experiment, the one with a concentration of 2.5 M and a volume of 4.8 L, and the initial solution is the one available of concentration 6.0 M. So, we need to know the volume of the initial solution we need to take to prepare the require solution. For the equation above we have:

Replacing the values:

Then, to prepare the solution needed for the experiment we must take 2.0 L of the H2SO4 stock solution of 6.0 M and dilute it to 4.8 L of solution, that is to say, add 2.8 L of water, so to get a 2.5 M H2SO4 solution.

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

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