Pre-Lab 7

Pre-Lab 7 - 3 + H + CO 2 + H 2 O + Na + 9. Distilled water...

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Frank Gervasi 10/18/10 Pre-Lab Experiment 7 1. It is unwise to haphazardly mix household chemicals because in the case of mixing ammonia and bleach, it would create a dangerous cloud of mustard gas. 2. NH 4 + can be detected by adding sodium hydroxide, NaOH, and noting the familiar odor of NH 3 or by the use of red litmus. 3. CO 3 2- can be detected when CO 2 gas is released from the substance after adding HCl. 4. The chloride ion reacts with H 2 SO 4 by releasing a pungent but colorless gas. 5. When mixed with BaCl 2 , the SO 4 2- ion will bind with Ba to create a precipitate. 6. The I - ion will bind to the silver and form a precipitate when mixed with AgNO 3 7. Ag+ can be detected by mixing it with NaCl, which causes the solid AgCl to be made ionically. 8. 2LiCl + H 2 SO 4 Li 2 SO 4 + 2HCl NH 4 + + OH - NH 3 + H 2 O AgNO 3 + I - AgI + NO 3 - NaHCO
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Unformatted text preview: 3 + H + CO 2 + H 2 O + Na + 9. Distilled water should be used in the lab instead of tap water because tap water is treated with chemicals that could cause unwanted reactions in the solutions we’re testing 10. If you were to add H2SO4 to a mixture of Na2CO3 and NaCl, you would not be able to detect the presence of Na2CO3 because the H from the acid would bind with the Cl from the salt, and nothing else. 11. 12. Dissolve the mixture in water. Then, add a little silver nitrate. Silver ions precipitate with chloride ions to form silver chloride. Then you could add some acid, like a little nitric acid. The carbonate ions will react with the protons to form carbonic acid, which will decompose into CO2 gas, and make bubbles....
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This note was uploaded on 11/07/2010 for the course 160 125 taught by Professor Rementer during the Fall '10 term at Rutgers.

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