Chapter 5, Problem 92IAE

Copper refining traditionally involves "roasting" insoluble sulfide ores (CuS) with oxygen. unfortunately, the process produces large quantities of ${\text{SO}}_{\text{2}}$ (g), whichis a major contributor to pollution and acid rain. An alternative process involves treating the sulfide ore with ${\text{HNO}}_{\text{2}}$ (g) which dissolves the CuS without generating any ${\text{SO}}_{\text{2}}$ . The unbalanced chemical expression for the reaction is given below.

$\text{CuS}\left(\text{s}\right){\text{+NO}}_{\text{3}}\left(\text{aq}\right)\to {\text{Cu}}^{\text{2+}}\left(\text{aq}\right)\text{+NO}\left(\text{g}\right){\text{+HSO}}_{\text{4}}\left(\text{aq}\right)$ (not balanced)

What volume of concentrated nitric acid solution is required kilogram of CuS? Assume that the concentrated nitric acid solution is 70% ${\text{HNO}}_{\text{2}}$ by mass and has a density of 1.40 g/mL.