What volume of 0.5 M is needed to neutralize 25 ml of 2 M H2SO4

What volume of 0.5 M is needed to neutralize 25 ml of 2 M H2SO4?
the answer is 200 ml. I am not sure why this answer, may be because I don't understand the concept of to neutralize. Please explain

the no. of h+(acidic) ions shold be equal to the no. o of OH-(basic) ions to completely neutralize the acid.(the soltion becomes neither acidic nor basic. or a neutral salt soln.)

the no. of moles of H2SO4 in 25ml of 2M soln. = Molarity x Volume = 2 x (25/1000)litres (as molarity is in terms of moles per litre)

=0.05 moles of h2so4. since each particle of h2so4 will give two ph+ ions

therfore no. of h+ ions = no of moles of h2so4 x 2
= 0.1 moles.

now same thing we apply for NaOH slution. each NaOH gives only 1 OH- ion.

no. of moles of OH- = N. of Moles of NaOH reqd. = NO. of moles of h+ for neutralisation.

the no Of moles of naoh or OH- = 0.5 x V ( v is the volume of naoh reqd.) = 0.1
therefore V = 0.2 litres. or 200ml.

phew. pls like the answer.

what is the base?
neutralization is a double replacement reaction
AH + BOH --> AB + H2O

0.025L x 2M = 0.05moles H2SO4 present
if the base has only one OH-:
2BOH + H2SO4 --> 2H2O + B2SO4 then it will take 0.1mole of base to neutralize the acid
1mole of 0.5M = 0.2L

if the base has 2 OH-:
B(OH)2 + H2SO4 --> BSO4 + 2H2O it will take 0.05moles of base to neutralize the acid
0.5moles of 0.5M = 0.1L

the volume of 0.5 to neutraliza 25 ml of 2 M H2O4 you need is 94756,3848758 ml of love