[AManWithNoPlan]

Why is A the answer? I figured the mass of Sulfuric Acid would come into play but my calculations only required converting Sodium Hydroxide (SO_4) to liters and multiplying it by the mols of SO_4.  So All I did was .3349 * .3946. I'm just suspicous of the simplicity.

[AWK]

Start from a balanced reaction of neutralization.

[Vidya]

write balanced equation ...
get moles of NaOH to moles of H2SO4 and finally divide it by total volume of the final solution.
Try it .

[docnet]

Because there are two moles of acid per mole of sulfuric acid. notice that it has two Hydrogen atoms that can be seperated from the molecule, each of them combining with the OH^- ion to form H₂O.  Therefore, when it's being titrated with a strong base such as NaOH, you can think of it as being twice as concentrated, so you would need half as much of it to get the job done. Hope this makes it easier.

EDITED

[billnotgatez]

...  strong acid such as NaOH,  ...

@docnet
Are you sure?

[docnet]

...  strong acid such as NaOH,  ...

@docnet
Are you sure?

 

Base! Sorry!


To the OP:

First of all, 39.46mL converts to .03946L and not .3946L.

Multiply the volume by the molarity to get the total number of moles of Base.

.3349M_base x .03946L_base = .01326 mol_base = .01326 mol_{acid titrated}

.01326mol_acid  / .0500L_acid = .2643M_acid.

Since there are two H+ ions per one sulfuric acid molecule, dividing .2643 by 2 gives us the answer, which is .1322 M_acid

Hope this helps