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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

Respuesta :

mathjohndough

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,

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

First we write a balanced equation,

[tex]H_2SO_4 + 2NaOH ==> Na_2SO_4 + 2H_2O[/tex].

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

[tex]31.26ml \times \frac{1L}{1000ml} \times \frac{0.621mol}{L} = 0.0194mol NaOH[/tex]

Using moles of [tex]NaOH[/tex] we find the molarity

[tex]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[/tex]

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



dsdrajlin

31.26 mL of 0.621 M NaOH is used to titrate 2.00 mL of 4.85 M H₂SO₄. with this concentration, we can conclude that the battery needs to be recharged.

A solution of unknown concentration of sulfuric acid is titrated with sodium hydroxide. The neutralization reaction is:

2 NaOH + H₂SO₄ ⇒ Na₂SO₄ + 2 H₂O

31.26 mL of 0.621 M NaOH react. The reacting moles of NaOH are:

[tex]0.03126 L \times \frac{0.621mol}{L} = 0.0194mol[/tex]

The molar ratio of NaOH to H₂SO₄ is 2:1. The reacting moles of H₂SO₄ are:

[tex]0.0194molNaOH \times \frac{1molH_2SO_4}{2molNaOH} = 0.00970 mol H_2SO_4[/tex]

0.00970 moles of H₂SO₄ are in 2.00 mL of solution. The molarity of H₂SO₄ is:

[tex]M = \frac{0.00970 mol}{0.00200L} = 4.85M[/tex]

Since the molarity of sulfuric acid in a fully charged car battery is 5.2 M and in a fully discharged battery is 4.8 M, the battery needs to be recharged.

31.26 mL of 0.621 M NaOH is used to titrate 2.00 mL of 4.85 M H₂SO₄. with this concentration, we can conclude that the battery needs to be recharged.

Learn more: https://brainly.com/question/23307058

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