Problem: 38. A solution was prepared by mixing 50.00 mL of 0.100 M HNO 3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

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We’re being asked to calculate the molarity (M) of nitric acid (HNO3) when 50.00 mL of 0.100 M HNO3 and 100.00 mL of 0.200 M HNO3 are mixed.


Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words:



We first need to determine the moles of HNO3 present in each initial solution. This is because we mixed two solutions containing HNO3 and the moles of HNO3 in the new solution is simply the sum of the moles of HNO3 in the original solutions.


Note that we need to convert mL to L since molarity is in mol/L.

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Problem Details

38. A solution was prepared by mixing 50.00 mL of 0.100 M HNO 3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

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Our tutors have indicated that to solve this problem you will need to apply the Molarity concept. You can view video lessons to learn Molarity. Or if you need more Molarity practice, you can also practice Molarity practice problems.

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Based on our data, we think this problem is relevant for Professor Oliver's class at UCSC.

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Our data indicates that this problem or a close variation was asked in Chemistry - Zumdahl 8th Edition. You can also practice Chemistry - Zumdahl 8th Edition practice problems.