Asample of battery acid is to be analyzed for its sulfuric acid content. a 1.00-ml sample weighs 1.227 g . this 1.00-ml sample is diluted to 250.0 ml, and 10.00 ml of this diluted acid requires 35.05 ml of 4.462×10−3 m ba(oh)2 for its titration. what is the mass percent of h2so4 in the battery acid?

The mass percent of in the battery acid is 31.9 %

Explanation:

We are given:

Molarity of solution =

Volume of solution = 35.05 mL

Putting values in above equation, we get:

By Stoichiometry of the reaction:

1 mole of barium hydroxide reacts with 1 mole of sulfuric acid

So, 0.00016 moles of barium hydroxide will react with = of sulfuric acid.

The calculated moles of sulfuric acid is present in 10 mL of solution.

To calculate the number of moles in 250 mL of solution, we use unitary method:

In 10 mL, the number of moles of sulfuric acid are 0.00016 moles

So, in 250 mL, the number of moles of sulfuric acid will be =

The calculated moles of sulfuric acid are present in 1 mL of solution.

Molar mass of sulfuric acid = 98 g/mol

Moles of sulfuric acid = 0.004 moles

Putting values in above equation, we get:

Mass of battery acid = 1.227 g

Mass of sulfuric acid = 0.398 g

Putting values in above equation, we get:

Hence, the mass percent sulfuric acid in battery acid is 31.9 %.

the electrical  conductivity  of asolution  of an electrolyte is measured by determining the resistance of thesolution  between two flat or cylindrical electrodes separated by a fixed distance.