How many grams of carbonic acid (H2CO3) would you need to make 1 liter of a 0.01M solution

Help please?
What formula do I use to solve this?
Is this a titration problem?

You would need magic to have any number of grams of H2CO3 because it does not exist in a molecular form. Carbonic acid is a fictitious acid, it does not exist as discrete molecules. What we call "carbonic acid" is actually a solution dissolved CO2 gas in equilibrium with H+ and HCO3- ions. Whoever wrote the original question is pulling your leg or doesn't know any better.

At 1L of 0;01mol/L solution, clearly, you would need 0.01 moles of "H2CO3". Feel free to multiply the molar mass of "H2CO3" by 0.01 to get the "mass". The molar mass of the nonexistent molecule is 62.0 g/mol. Therefore, you would need 0.62g of the fictitious acid.

========== Follow up ==========

Jacob is off by a factor of 10, and "no", it's not a titration problem.

conc*vol=mol
0.01*0.1=0.001
mol*mr=mass
0.001*(2+12+16*3)=0.062 grams