For the reaction, state if the reaction is quantitative, or, if not, state whether products or reactants are favoured at equilibrium.

Question

1. 100 mL of 0.1 mol/L nitric acid reacts with 100 mL of 0.1 mol/L ammonium hydrogen carbonate

My question is how do I know if it is quantitive or not. and if its not how do I know if it is favoured at equilibrium? Can u please help asap...I need to hand this in today.

The equation is the key. Write the equation and balance it.
HNO3 + NH4HCO3 ==> H2CO3 + NH4NO3.

The H2CO3 is not stable and continues as follows:
H2CO3(aq) ==> H2O(l) + CO2(g) so that the overall reaction is

HNO3(aq) + NH4HCO3(s) ==> H2O(l) + CO2(g) + NH4NO3(aq)

A reaction goes to completion if
a. a precipitate is formed.
b. a gas is formed (and escapes;i.e., it isn't in a closed system).
c. a slightly ionized substance is formed.

Does this help?

Thanks!