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what is the normality of a 1.5 M solution of sulfuric acid

Sagot :

Answer:

3N of sulfuric acid.

Explanation:

Remember that normality is a measure of concentration equal to the gram equivalent weight per liter of solution.

First, let's see the equation of normality:

[tex]Normality=Molarity\cdot\frac{molecular\text{ mass of solute}}{Equivalent\text{ mass of solute}}.[/tex]

And let's see that sulfuric acid (H2SO4) is a diprotic acid because it contains 2 protons in its structure (2H+), so we're going to use this value to calculate the equivalent mass of solute.

Now, let's replace the given data: molarity is 1.5 M, the molecular mass of solute is the molecular mass of H2SO4 which is 98 g/mol (you can calculate the molecular mass of a compound using the periodic table) and the equivalent mass of solute is the division between molecular mass and the number of protons, in this case, 2:

[tex]Normality=1.5M\cdot\frac{98\text{ }\frac{g}{mol}}{\frac{98\text{ }\frac{g}{mol}}{2}}=1.5\cdot\frac{98}{49}=3\text{ N.}[/tex]

The normality of this solution would be 3N.

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