sulphuric acid is diprotic (2 H⁺)
so the normality is twice the molarity
so the normality is twice the molarity
Sulphuric acid (H2SO4) is a diprotic acid, meaning that each molecule of H2SO4 can donate two hydrogen ions (H+). Therefore, the number of equivalents (n) of sulphuric acid is twice the number of moles (m) present in the solution.
To calculate the number of equivalents (n), you can use the formula:
n = m × valence
where:
m = moles of solute
valence = number of ions per molecule
For sulphuric acid, the valence is 2 because it donates two hydrogen ions. The moles of sulphuric acid can be found using the formula:
m = M × V
where:
M = molarity of the solution
V = volume of the solution in liters
In this case, the molarity of the sulphuric acid solution is given as 1.5M.
Let's assume the volume of the solution is 1 liter:
m = 1.5M × 1L = 1.5 moles
Now we can calculate the number of equivalents (n):
n = 1.5 moles × 2 = 3 equivalents
Therefore, the normality of a 1.5M sulphuric acid solution is 3N.
In the case of sulfuric acid (H2SO4), it is a diprotic acid, which means it can donate two protons (H+ ions) per molecule. So, to calculate the normality, we need to multiply the molarity (M) of the sulfuric acid by the number of protons it donates.
In this case, the molarity (M) of the sulfuric acid is given as 1.5 M. Since sulfuric acid donates two protons per molecule, we multiply the molarity by 2 to get the normality:
Normality (N) = Molarity (M) × Number of protons donated
Normality (N) = 1.5 M × 2
Normality (N) = 3 N
Therefore, the normality of a 1.5M sulfuric acid solution is 3N.