Problem: Consider the given graph. If the given graph shows the titration of 23.00 mL of an HNO3 solution of an unknown concentration with a 0.135 M LiOH solution, what is the molarity of the acid solution?

FREE Expert Solution
FREE Expert Solution

We’re being asked to calculate the molarity of HNO3 (strong acid) from the given titration data with LiOH (strong base)


Recall that in the titration of a strong acid and strong base, the equivalence point occurs at pH 7. From the titration curve, we can determine the volume of LiOH:



This means that 23.00 mL of HNO3 required 20.00 mL of 0.135 M LiOH to reach the equivalence point.


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Problem Details

Consider the given graph. If the given graph shows the titration of 23.00 mL of an HNO3 solution of an unknown concentration with a 0.135 M LiOH solution, what is the molarity of the acid solution?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equivalence Point concept. If you need more Equivalence Point practice, you can also practice Equivalence Point practice problems.

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