Well, I'm glad you didn't ask me to calculate how many clowns can fit into a car, because that's a whole different kind of chemistry! But hey, let's tackle this acid problem together.
First, we need to find the number of moles of HNO3 we need. The concentration of the solution is given as 3.00 mol dm-3, and the volume is 2.00 dm3. So, we can use the formula:
moles = concentration x volume
moles = 3.00 mol dm-3 x 2.00 dm3
moles = 6.00 mol
Alright, now we know we need 6.00 moles of HNO3. But the concentration of the nitric acid is given as 19.0% by mass. So, we need to find the mass of HNO3 first.
To find the mass, we can use the formula:
mass = concentration x volume x molar mass
mass = 0.190 x 2.00 dm3 x 63 g/mol
mass = 24.06 g
Ah, math! It certainly knows how to keep us on our toes. Now that we have the mass, we can calculate the volume of the acid needed. We know that the density of the acid is 1.11 g cm-3, which is equivalent to 1.11 g/mL.
volume = mass / density
volume = 24.06 g / 1.11 g/mL
volume = 21.7 mL
Oh, we're so close! But wait, we need to convert mL to dm3 since that's what the question is asking for. Remember that 1 dm3 is equal to 1000 mL.
volume = 21.7 mL / 1000
volume = 0.0217 dm3
And there you have it! The volume of nitric acid needed to prepare 2.00 dm3 of 3.00 mol dm-3 HNO3 solution is approximately 0.0217 dm3. Now that's an acid solution to the problem!