Calculating Normality after Mixing M/10 H2SO4 and M/10 NaOH
- First, calculate the number of moles of H2SO4 in 100 ml M/10 solution:
- Molarity (M) = 10^-1 M
- Volume (V) = 100 ml = 0.1 L
- Moles = M x V = 10^-1 x 0.1 = 10^-2 moles
- Next, calculate the number of moles of NaOH in 500 ml M/10 solution:
- Molarity (M) = 10^-1 M
- Volume (V) = 500 ml = 0.5 L
- Moles = M x V = 10^-1 x 0.5 = 0.05 moles
- Determine the limiting reactant by comparing the moles of H2SO4 and NaOH:
- H2SO4:NaOH ratio = 1:2 (from the balanced equation)
- Since NaOH has fewer moles, it is the limiting reactant
- Calculate the remaining moles of NaOH after reacting with all the H2SO4:
- Remaining moles = Initial moles - moles used in reaction = 0.05 - 0.01 = 0.04 moles
- Calculate the new volume of the final solution after mixing:
- Total volume = Volume of H2SO4 + Volume of NaOH = 100 ml + 500 ml = 600 ml = 0.6 L
- Finally, calculate the Normality of the final solution:
- Moles of NaOH remaining = 0.04 moles
- Normality = Moles of solute / Volume of solution in liters
- Normality = 0.04 / 0.6 = 0.0667 N
Therefore, the Normality of the final solution after mixing M/10 H2SO4 with M/10 NaOH is 0.0667 N.

Normality=no of gram eqvalent/n factor