For the given reaction:
$CaCO_{3} + 2HCl \to CaCl_{2} + H_{2}O + CO_{2}$
If $90 \ g$ of $CaCO_{3}$ is added to $300 \ mL$ of $HCl$ solution which contains $38.55\%$ $HCl$ by mass and has a density of $1.13 \ g \ mL^{-1}$,then which of the following options is correct?
[Given molar masses of $H$,$Cl$,$Ca$,and $O$ are $1$,$35.5$,$40$,and $16 \ g \ mol^{-1}$ respectively]

• A
  $64.97 \ g$ of $HCl$ remains unreacted
• B
  $32.85 \ g$ of $CaCO_{3}$ remains unreacted
• C
  $97.30 \ g$ of $HCl$ reacted
• D
  $60.32 \ g$ of $HCl$ remains unreacted