$1)$ Ascorbic acid reacts with iodine in solution based on the following reaction.

$C_6{H}_8{O}_{6(aq)}+I_{2(aq)}{C}_6{H}_6{O}_{6(aq)}+2H_{(aq)}^{+}+2I_{(aq)}$

The iodine titrant has a concentration of $2\mathrm{.}00{10}^{-3mo\frac{l}{L}}$and was titrated with $10\mathrm{.}0mL$ samples of boxed orange juice.

Answer the questions below. The data is as follows:

$\backslash$table$[[$Trial$,1,2,3,4],[$Final burette reading $(mL),11\mathrm{.}08,21\mathrm{.}27,31\mathrm{.}50,41\mathrm{.}72],[$Initial burette reading $(mL),0\mathrm{.}05,11\mathrm{.}03,21\mathrm{.}27,31\mathrm{.}50],[$Volume of titrant added $(mL),11\mathrm{.}03,10\mathrm{.}24,10\mathrm{.}23,10\mathrm{.}22],[$Indicator colour starch solution$),$Purple,Blue,Blue,Blue$]]$

a$.$ Calculate the concentration of ascorbic acid in the orange juice sample.

b$.$ If the juice box is $200mL,$ how many moles of ascorbic acid are present in the whole juice box?

c$.$ The Canadian government recommends a daily consumption of $60mg$ of vitamin $C.$ How does this compare to having one juice box a day?