1. Weigh out about 0.5 grams of solid copper wire into a 250-mL beaker, recordin

Question

1. Weigh out about 0.5 grams of solid copper wire into a 250-mL beaker, recording in your notebook the precise mass to the nearest milligram. [Include this mass in your lab report.] In a fume hood, place the beaker on a wire square (gauze) supported on an iron ring attached to a ring stand and cautiously add 15 mL of 6 M nitric acid [HNOMaq) If the copper does not begin to react within a reasonably short time, gently heat the nitric acid with your Bunsen burner to initiate the reaction, but be sure to stop heating before all the solution is vaporized! The copper should react completely and "disappear" into solution. Record what you observe as this reaction and all subsequent reactions occur [1] Cu(s) + 4HINO3(ag)- Cu(NO3)2(ag) + 2NO2(g) + 2H20 Question: What observation supports the fornation of the Cu-+ ions in the solution? Question: Why was it important to perform this reaction in the fume hood? Question; Is there any copper metal left after you have completed this step? If not where is the copper?

Explanation / Answer

Q1.

copper (II) ions will be blue in solution

Q2

we need to get any HNO3 fumes formed, which are very irritating to respiratory tract

Also, some NO2 / NO3 gases could form

Q3

if excess acid is used, thre should not be solid Copper present

Also, note that coppr will not dissapear, it will simply just go as Cu2+ into solution

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