Question

In: Chemistry

What safety concerns are there for dissolving the copper with concentrated nitric acid?

What safety concerns are there for dissolving the copper with concentrated nitric acid?

Solutions

Expert Solution

This reaction is interesting to watch as well as to perform it. Safety concerns are to be observed to do any chemical experiments in the laboratory or outside.

The chemicals required for the above reaction to take place are copper and conc.nitric acid. Copper by nature is not harmful unless the individual is exposed to higher levels of copper. copper is available in the environment naturally through decay of vegetables, burning of leaves and so on. Our body needs trace amounts of copper but higher level of exposure by breathing in copper will cause irritation to nose and throat and ingesting copper may lead to vomiting, kidney damage and death. Therefore, While doing chemical experiments it is mandatory to perform it careful by wearing gloves. The other reagent is Conc.Nitric Acid and its vapors are highly corrosive and affects the eyes, skin and mucous membranes. It oxidizes very fast in air, hence wear goggles or face shield and use nitrile gloves while handling it.

As the reaction is happening while adding copper to conc nitric acid, nitrogen dioxide is evolved, which is very toxic therefore, the reaction can be performed in a fume hood or in a open ventilation area. As the water in the vessel will help in dissolving nitrogen dioxide and diffusion of nitrogen dioxide can be controlled by using a a piece of glass wool in the neck of the flask. ( handle glass wool using forceps).

Note: Before doing the experiments, please check the apparatus and make sure there are no cracks or faults.


Related Solutions

Redox Reactions: Less active metals like copper will reacti with concentrated nitric acid to produce nitric...
Redox Reactions: Less active metals like copper will reacti with concentrated nitric acid to produce nitric oxide gas and the Cu2+(aq) ion at 25C. A) Write balanced chemical equation for this process.               6H+(aq) + 2HNO3(aq) + 3Cu(s) --> 3Cu2+(aq) + 2NO(g) + 4H2O (aq) B) Evaluate change in E for the reaction in (a).
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and...
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much concentrated solution would you take to prepare 1.00 L of 0.115 M HNO3 by mixing with water?
A concentrated nitric acid solution has a density of 1.41 g/mL at 25C and is 15.8...
A concentrated nitric acid solution has a density of 1.41 g/mL at 25C and is 15.8 M. What is the percent by mass of HNO3 in the solution? a. 70.6 % HNO3 by mass b. 1.12% c. .895 % d. 1.77 % e. 44.7% how do i identify which one is the solute and solvent of the two numbers given? and the correct answer is supposedly 70.6% from the solution :) thank you for you help!
You can purchase nitric acid in a concentrated form that is 70.3% HNO(3) by mass and...
You can purchase nitric acid in a concentrated form that is 70.3% HNO(3) by mass and has a density of 1.41 g/mL. Describe exactly how to prepare 1.15 L of 0.100 M HNO(3) from the concentrated solution. Please explain thoroughly.
(A) Calculate the molarity of commercially available concentrated nitric acid reagent given the following data: Molecular...
(A) Calculate the molarity of commercially available concentrated nitric acid reagent given the following data: Molecular formula: HNO3 Molar mass = 63.01 g/mol Purity/Reagent Concentrate: 70.9% (w/w) Specific gravity @20 degrees Celsius = 1.423 (Hint: Using the specific gravity, calculate the mass of one liter solution. Of this mass, only 70.9% is pure HNO3; the remainder being water). (B) To make 212 mL of 0.15 M solution of nitric acid, what volume of the concentrated nitric acid will be needed?...
in my chem lab brass and nitric acid reacted to form copper ions and I had...
in my chem lab brass and nitric acid reacted to form copper ions and I had to calculate the percent copper in the brass. I came out with a percentage of 36%. It was expected that the copper int he brass percentage would be higher. So what could be some likely causes of experimental error for the percentage of copper in brass to be much lower?
Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in concentrated...
Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in concentrated NaOH(aq). Calculate the amount of Ga(s) that can be deposited from a Ga(III) solution using a current of 0.360 A that flows for 20.0 min.
Suppose a solution is prepared by dissolving 15.0g NaOH in 0.150 L of 0.250 M nitric...
Suppose a solution is prepared by dissolving 15.0g NaOH in 0.150 L of 0.250 M nitric acid. What is the final concentration of OH- ions in the solution after the reaction has gone to completion. Assume that there is no volume change when adding the grams of NaOH.
when compounds are nitrated, typicallya mixture of concentrated nitric and sulfuric acids are required. howerever, when...
when compounds are nitrated, typicallya mixture of concentrated nitric and sulfuric acids are required. howerever, when phenol undergoes nitration only dilute nitric acid is required. why is this?
Nitrogen dioxide is used industrially to produce nitric acid, but it contributes to acid rain and...
Nitrogen dioxide is used industrially to produce nitric acid, but it contributes to acid rain and photochemical smog. What volume of nitrogen dioxide is formed at 791 torr and 28.2°C by reacting 3.85 cm3of copper (d = 8.95 g/cm3) with 240. mL of nitric acid  (d = 1.42 g/cm3, 68.0% HNO3 by mass)? Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) ______ L NO2
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT