nPart 1 we used nitric acid to oxidize the solid copper and drive it into soluti

Question

nPart 1 we used nitric acid to oxidize the solid copper and drive it into solution as the Cu2+ ion. Show that the 4.0 mL of nitric acid used was an excessive amount by calculating the volume (in mL) of 16 mol/L nitric acid solution needed to completely react 0.525 g of solid copper. Start this problem by copying the balanced chemical equation for this reaction to ensure you use the correct stoichiometry in this calculation. Balanced molecular form of the chemical equation for copper solid reacting with nitric acid solution

Explanation / Answer

Here, according to chemical equation, it can be easily observed that

1 mole of Solid Copper reacts with 4 moles of Nitric acid.

Now, 0.525 g of Copper means

moles of Copper = 0.525/Mw = 0.525/63.546 = 8.2617 millimoles.

Hence, moles of Nitric acid required = 4*8.2617 = 33.0468 millimoles.

Given, concentation of nitric acid = 16 moles per litre or 16 millimoles per millilitre of solution.

Now, volume required = 33.0468/16 = 2.065425 mL which is less than 4 mL.

Hence, 4 mL would have been in excess.  

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