What mass of ammonium thiocyanate (nh4scn) must be used if it is to react completely with 5.7 g barium hydroxide octahydrate?

The balanced chemical equation is represented as:

Ba (OH) 2·8 H2O + 2 NH4SCN = Ba (SCN) 2 + 10 H2O + 2 NH3

To determine the mass of ammonium thiocyanate needed completely react, we use the amount given of the other reactant. Then, convert to moles by the molar mass. And using the relations of the substances in the reaction, we can determine the amount of ammonium thiocyanate.

moles Ba (OH) 2·8 H2O = 5.7 g Ba (OH) 2·8 H2O (1 mol / 315.46 g) = 0.0181 mol Ba (OH) 2·8 H2O

moles NH4SCN = 0.0181 mol Ba (OH) 2·8 H2O (2 mol NH4SCN / 1 mol Ba (OH) 2·8 H2O) = 0.0361 mol NH4SCN

mass NH4SCN = 0.0361 mol NH4SCN (76.122 g / 1 mol) = 2.75 g NH4SCN