What is the concentration of sulfuric acid in car batteries

Asked by admin @ 05/11/2021 in Chemistry viewed by 268 People

The molarity of sulfuric acid in a fully charged car battery is 5.2 m. when fully discharged the molarity is 4.8m. a 2.00ml sample of battery acid was titrated with 31.26ml of

a.621 m sodium hydroxide solution. does the battery need to be recharged

Answered by admin @ 05/11/2021

This question requires utilization of the equivalence point of a reaction, which is a point in the chemical reaction where the two solutions have been mixed in exactly the right proportions. This means that,

$M_1V_1=M_2V_2$ , where $M_1$ is the molarity of the acid sulfuric acid, $V_1$ the volume of acid, $M_2$ is the molarity of the base sodium hydroxide and $V_2$ is the volume of the base.

First we write a balanced equation,

$H_2SO_4 + 2NaOH ==> Na_2SO_4 + 2H_2O$ .

The stochiometric ratio of $H_2SO_4: NaOH$ is 1:2. Which means 1 mol $H_2SO_4$ react with 2 mol $NaOH$ . Using the volume and molarity of $NaOH$ given we find the molarity of $H_2SO_4$ .

$31.26ml \times \frac{1L}{1000ml} \times \frac{0.621mol}{L} = 0.0194mol NaOH$

Using moles of $NaOH$ we find the molarity

$0.0194mol NaOH \times \frac{1mol H_2SO_4}{2mol NaOH} \times \frac{1 mol}{2.0ml} \times \frac{1000ml}{L} = 4.8 M H_2SO_4$

It is fully discharged so the battery needs to be recharged.

What is the concentration of sulfuric acid in car batteries

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