Final answer:
To find the volume of 0.132M HNO₃ solution that will react with 33.2ml of a 0.108m Na₂CO₃ solution, a stoichiometric calculation based on the balanced chemical equation is needed.
Step-by-step explanation:
To determine the volume of 0.132M HNO₃ solution required to completely react with 33.2ml of a 0.108m Na₂CO₃ solution, we need to use the concept of stoichiometry from chemistry, which involves the quantitative aspects of chemical reactions.
First, write down the balanced chemical equation:
2 HNO₃ (aq) + Na₂CO₃ (aq) → 2 NaNO₃ (aq) + H₂O (l) + CO₂ (g)
We can see from the balanced equation that 2 moles of HNO₃ react with 1 mole of Na₂CO₃. Next, calculate the number of moles of Na₂CO₃:
moles Na₂CO₃ = 33.2mL * 0.108M = moles
Now, use the mole ratio from the balanced equation to find the moles of HNO₃:
moles HNO₃ = 2 * moles Na₂CO₃
Finally, calculate the volume of HNO₃ required using its molarity:
volume HNO₃ (mL) = moles HNO₃ / Molarity of HNO₃
Perform the actual calculations to get the final volume in milliliters.