Acid$-$base titration

$13-25\mathrm{.}0mL$ of sulfuric acid $H_{2}S{O}_4$ solution was titrated with $45\mathrm{.}0mL$ of $0\mathrm{.}88$MNaOH solution to produce $N{a}_{2}S{O}_4.$ Calculate the concentration of sulfuric acid in molL of solution $($Molar mass of $H_{2}S{O}_4=98\mathrm{.}0g(mol).$

$2$NaOH$+H_{2}S{O}_{4}N{a}_{2}S{O}_4+2H_{2}O$

a$)0\mathrm{.}79$

b$)0\mathrm{.}66M$

c$)0\mathrm{.}54M$

d$)0\mathrm{.}50M$