Week #2 Post Lab
1.) Define the following: electrolyte, nonelectrolyte
Electrolyte: A substance that dissolves in water to form solutions that conduct electricity. Nonelectrolyte: A compound that doesn’t dissociate into ions when dissolved in water. 2.) Using examples in the last link, draw beakers showing atomic scale representations of aqueous solutions of the following compounds. Classify each as an electrolyte or nonelectrolyte. * Ba(OH)2 (aq)
* NH3 (aq)
* C3H7OH (aq)
* NaHCO3 (aq)
3.) Why would it be important to use de-ionized water when preparing the aqueous solutions in this experiment? It is important to use de-ionized water in this experiment because you don’t want the electrolytes in the water to affect the aqueous solutions conduct an electric current, especially if it can’t. 4.) Pick an area of science that interests you and describe how the concept of electrolytes is used in that particular field. In physiology, all higher life forms require a complex electrolyte balance between the intracellular and extracellular environment. In particular, the maintenance of osmotic gradients of electrolytes is important. Such gradients affect and regulate the hydration of the body, blood pH, and are critical for nerve and muscle function. 5) According to your experiment and the reading, answer the following. * Is HI a strong, weak, or non-electrolyte? Explain
HI is a strong electrolyte because it will react with H2O to form large concentrations of ions of H+ and I- * Is HI an ionic compound? Why or why not?
HI isn’t an ionic compound. It is a covalent compound because both hydrogen and iodine are nonmetals. 6) Why would the bulb light up when placed in an aqueous solution of sodium chloride but not in a solid sample of sodium chloride?
In a solid sample of sodium chloride, sodium and chloride are bonded together ionic and so there aren’t any free electrons to support the flow of electricity. When sodium chloride is...
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