What mass of sodium carbonate is required to react with a 1*L volume of nitric acid, whose concentration is 15*mol*L^-1?

1 Answer
Jan 30, 2017

You need to specify the concentration, the molarity of the nitric acid.

Explanation:

Concentrated nitric acid, is approx. a 15*mol*L^-1 solution. I will assume you are using this stuff (in fact, the concentration would not be issued to A level students, so you will have to adjust your answer appropriately).

We need (i) a stoichiometrically balanced equation:

Na_2CO_3(aq) + 2HNO_3(aq) rarr 2NaNO_3(aq) + H_2O(l) + CO_2(g)uarr

Mass and charge are balanced as required, and (ii), equivalent quantitites of acid:

"Moles of nitric acid" = 1*Lxx15*mol*L^-1=15*mol.

Given the stoichiometry of the equation, this will neutralize "HALF an equiv" of Na_2CO_3, and thus 7.5*mol.

This has an equivalent mass of 7.5*molxx105.99*g*mol^-1=794.9*g.