Problem: If 23.9 mL of the strontium hydroxide solution (1.47 M)  was needed to neutralize a 31.5 mL aliquot of the nitric acid solution, what is the concentration (molarity) of the acid?

FREE Expert Solution

We are being asked to calculate the concentration (molarity) of the acid if 23.9 mL of strontium hydroxide solution was needed to neutralize a 31.5 mL aliquot of nitric acid solution.


Strontium hydroxide, Sr(OH)2, is a strong base. Nitric acid, HNO3, is a strong acid

So, the titration of nitric acid solution with strontium hydroxide solution is a strong acid strong base titration.


The chemical equation of the reaction is

Sr(OH)2(aq) + HNO3(aq) Sr(NO3)2(aq) + H2O(l)



During titration, Sr(OH)2 reacts with 2 HNO3

The amount of HNO3 in the solution can be determined by the total amount of Sr(OH)2 used. 


We’re going to calculate for the concentration of HNO3, using the following steps:

1. Calculate moles of Sr(OH)2

2. Determine moles of HNO3

3. Calculate the concentration of HNO3


Recall: 

Molarity (M)= mol L


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Problem Details

If 23.9 mL of the strontium hydroxide solution (1.47 M)  was needed to neutralize a 31.5 mL aliquot of the nitric acid solution, what is the concentration (molarity) of the acid?

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