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what volume in ml of a 0.132m HNO₃ solution will completely react wihth 33.2ml of a 0.108m Na₂CO₃ solution?

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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.

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