Question

20 ml of a 0.125 N HCl solution were neutralised by 25 ml of a KOH solution. What is the normaility of KOH solution​

Answer 1

Your Question:

What is the normality of the KOH solution, 20.0 mL of which is neutralized by 16 mL of 0.125 M H2SO4?

Answer :

Balanced equation:

2KOH(aq) + H2SO4(aq) → K2SO4(aq) + 2H2O(l)

2mol KOH react with 1 mol H2SO4

Mol H2SO4 in 16mL of 0.125M solution = 16mL /1000mL/L * 0.125mol /L = 0.002 mol

This will react with 0.002*2 = 0.004 mol KOH

20.0mL KOH solution contains 0.004 mol KOH

1000mL = 1.0L KOH solution contains :

Mol KOH /L = 1000mL/L /20mL * 0.004 mol = 0.20mol/L

Normality of KOH solution = molarity of KOH solution = 0.20N