Question

What volume of a 1.420 M NaOH solution is required to titrate 25.00 mL of a 4.50 M H,SO, solution?

Answer 1

Solution:

$Chemical\; reaction:$

$H_2SO_4(aq)\;+\;2NaOH(aq)\implies Na_2SO_4(aq)\;+\;H_2O(l)$

1) By using the acid-base equation:

$M_1V_1=M_2V_2$

$4.5M*25ml=1.42M*V_2$

$V_2=\frac{(4.5M*25ml)}{1.42M}$

Remember 1 mole H₂SO₄ is equivalent to 2 moles NaOH, that is Normality of H₂SO₄ = (Molarity x 2)

$79.2*2ml=158ml\;of\;1.42M\;NaOH\;will\;be\;required.$

Answer:

$V_2=158.4ml$