Can someone help me with this I’m trying to review for my test but still don’t understand how to to this, thank you! In this lab, you will be determining the mass percent of copper in a sample of brass. You will first be adding nitric acid to the brass, which will react with the copper and the zinc in the brass sample (thus dissolving it). This results in a colorless solution of zinc nitrate and a deep blue solution of copper(II) nitrate. The equation for the formation of copper(II) nitrate is shown below.

Balanced molecular equation: 4 HNO3(l) + Cu(s) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O(l)

Balanced net ionic equation: 4 H+(aq) + 2 NO3–(aq) + Cu(s) → 2 NO(g) + 2 H2O(l) + Cu2+(aq)

Assuming you start with a 2g sample of brass and assuming your brass sample is 100% copper, calculate the minimum volume (in mL) of concentrated 15.8M HNO3(aq) that needs to be added to react completely with the brass (assumed to be 100% copper for now). Note: the moles of H+(aq) represent the moles of HNO3(aq) reacted in the balanced equation above.