**$\mathbf{35}\mathbf{.}\mathbf{1}\mathbf{}\overline{)\mathbf{mL}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}}\mathbf{}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}\overline{)\mathbf{L}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mL}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}}}\mathbf{\times}\frac{\mathbf{0}\mathbf{.}\mathbf{112}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{L}\mathbf{}{\mathbf{Na}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}}}$ **

**= 3.9312x10 ^{-3} mol Na_{2}CO_{3}**

What volume (in mL) of a 0.175 M HNO_{3} solution is required to completely react with 35.1 mL of a 0.112 M Na_{2}CO_{3} solution according to the following balanced chemical equation?

Na_{2}CO_{3}(aq) + 2 HNO_{3}(aq) → 2 NaNO_{3}(aq) + CO_{2}(g) + H_{2}O(l)

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