I keep getting the wrong answer for this Molarity problem

Automobile batteries use 3.0 M H2SO4 as an electrolyte. How much 1.20 M NaOH will be needed to neutralize 225mL of battery acid?

I keep getting 0.09L but the answer is 1.1L

1) Calculate moles of H2SO4

0.225 L x 3.0 mol / L = 0.675 mol H2SO4

2) Calculate moles of NaOH needed.

The equation
H2SO4 + 2 NaOH -----> Na2SO4 + 2 H2O
shows that the mole ratio of NaOH to H2SO4 is 2 to 1

0.675 mol H2SO4 x 2 NaOH / 1 H2SO4 = 1.35 mol NaOH needed

3) Calculate volume of NaOH needed

1.35 mol NaOH x 1 L / 1.20 mol = 1.125 L or 1.1 L