Question

It take 38.70cm³ of 1.90m NaoH to neutralize 10.30cm³ of H2so4 in a battery, calculate the molar concentration of H2so4

Answer 1

`M_(acid)=3.57M`

Step-by-step explanation:

Hello there!

In this case, since this acid-base neutralization is performed in a 1:2 mole ratio of acid to base as the former is a diprotic acid (two hydrogen ions in the molecule), we can write the following equation:

`2M_(acid)V_(acid)=M_(base)V_(base)`

In such a way, we can solve for the molarity of the acid, given the molarity and concentration of the NaOH base and the volume of the acid:

`M_(acid)=(M_(base)V_(base))/(2V_(acid))`

Thus, we plug in the given data to obtain:

`M_(acid)=(38.70cm^3*1.90M)/(2(10.30cm^3)) \\\\M_(acid)=3.57M`

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