A #75*mL# volume of #0.100*mol*L^-1# #HNO_3(aq)# and a #50*mL# volume of #0.150*mol*L^-1# #Ba(OH)_2(aq)# are mixed...will the reaction proceed quantitatively...?

Question

Natalie Anton · Accepted Answer

We need (i) a stoichiometric equation:

#Ba(OH)_2(s) + 2HNO_3(aq) rarr Ba(NO_3)_2(aq) + 2H_2O(l)# and require (ii) comparable amounts of the reagents we employ: #"Moles of nitric acid:"# #75xx10^-3*Lxx0.100*mol*L^-1# #= 7.50xx10^-3*mol#. #"Moles of barium hydroxide:"# #50xx10^-3*Lxx0.150*mol*L^-1# #= 7.50xx10^-3*mol#. And thus there is an equivalent quantity of #1.50xx10^-2*mol# hydroxide ion. Why? This means that the question should never have been asked in the first place. In addition, since barium hydroxide is highly soluble, the question should have asked for an equivalent amount of sodium or potassium hydroxide instead of the given volume and quantity of nitric acid, which will not neutralize the given quantity of barium hydroxide.

Noah Aldrich · Answer

undefined To determine if the reaction will proceed quantitatively, first, write the balanced chemical equation for the reaction between HNO3 and Ba(OH)2. Then calculate the number of moles of each reactant present in the mixture. Use stoichiometry to determine the limiting reactant and the theoretical yield of the product. If the reactants are mixed in stoichiometric ratios, the reaction will proceed quantitatively.