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12.5 mL of a solution containing 6g of a dibasic acid in 1L was found to be neutralised by 10mL of a decinormal solution of NaOH. The molecular mass of the acid is:
(a110
(b)75
(c)120
(d)150

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Last updated date: 13th Jun 2024
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Answer
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Hint:Neutralisation is the process where a known quantity of acid and a base react to form salt and water. Using stoichiometric calculation we can solve the question.

Complete step by step answer
It is given that the amount of acid in 1L solution = 6g
So, the amount of acid in 12.5mL solution will be = \[\dfrac{6}{1000}\times 12.5g=0.075g\]
When it is at neutralisation,
10mL of \[\dfrac{N}{10}\]NaOH = 10mL of \[\dfrac{N}{10}\]acid (it is given that decinormal which means\[\dfrac{N}{10}\])
We calculated that \[\dfrac{N}{10}\]acid=0.075g
So, for 1000mL \[\dfrac{N}{10}\]acid=\[\dfrac{0.075}{10}\times 1000=7.5\]g
1000mL of N acid = 7.5x10 =75g
Therefore, we get the equivalent mass of the acid= 75
As the acid is dibasic, we need to multiply equivalent mass with 2 in order to calculate molecular mass.
Molecular mass= 75x2=150g
Thus, the correct answer to the question is option (d).

Additional Information:
Neutralisation reactions can be used for quantitative analysis of compounds. Either acid or base quantity would be known, that is it is fixed and we can find the quantity of the other. This question is one example for such analysis. It has many applications in industry and laboratories. In wastewater treatment, chemical neutralisation methods are used to decrease the damage caused by an effluent upon its release into the environment.

Note:
Only in neutralisation reaction we can take the condition 10mL of \[\dfrac{N}{10}\]NaOH = 10mL of \[\dfrac{N}{10}\]acid. We should also keep in mind to multiply the equivalent mass with 2, and then only we get the molecular mass.