Electrolytes
Chemistry Demo Lab
Prepared for: Prof. Jared Gilmore
By: James Loquellano
Date. . . . .
LIGHT BULB EXPERIMENT
Ion - an electrically charged atom or group of atoms formed by the loss or gain of one or more electrons.
Ionization - The condition of being dissociated into ions by heat, electrical discharge, radiation, or chemical reaction.
Electrolyte - A chemical compound that ionizes when dissolved or molten to produce an electrically conductive medium.
Dissociation - When an ionic compound breaks up into its ions.
The experiment started by placing the rods of the light bulb device into the beaker in which contained 200 ml of distilled water , whether to test if the light bulb will come on. The light bulb did not light on because pure water does not conduct electricity. However, when the light bulb tester was put into a beaker of tap water, it did light on. The only difference between the two is that electrolytes are removed in distilled water, creating imbalance of electrolytes thus resulting a low electrical current. The second time around, ½ teaspoon of NaCl was added and stirred in distilled water and still no light, but when added more of table salt (NaCl) the light bulb lighted up. The reason it lighted up when more table salt was added, was because it was dissolved in the water and dissociated into charged particles, the ions of sodium and chlorine, which now allow the solution to conduct electricity through its positive and negative charges. So the ionic substance table salt is a strong electrolyte. And that proves that the first attempt didn’t have enough of the ions from NaCl to conduct electricity.
The experiment was repeated using table sugar instead of salt. The term non-electrolyte refers to a substance which dissolves in water but does not allow electrical conductivity. As the sugar dissolves, the light did not light up. So sugar is a non-electrolyte.
Some acids and bases are also strong electrolytes. The next example was
Prepared for: Prof. Jared Gilmore
By: James Loquellano
Date. . . . .
LIGHT BULB EXPERIMENT
Ion - an electrically charged atom or group of atoms formed by the loss or gain of one or more electrons.
Ionization - The condition of being dissociated into ions by heat, electrical discharge, radiation, or chemical reaction.
Electrolyte - A chemical compound that ionizes when dissolved or molten to produce an electrically conductive medium.
Dissociation - When an ionic compound breaks up into its ions.
The experiment started by placing the rods of the light bulb device into the beaker in which contained 200 ml of distilled water , whether to test if the light bulb will come on. The light bulb did not light on because pure water does not conduct electricity. However, when the light bulb tester was put into a beaker of tap water, it did light on. The only difference between the two is that electrolytes are removed in distilled water, creating imbalance of electrolytes thus resulting a low electrical current. The second time around, ½ teaspoon of NaCl was added and stirred in distilled water and still no light, but when added more of table salt (NaCl) the light bulb lighted up. The reason it lighted up when more table salt was added, was because it was dissolved in the water and dissociated into charged particles, the ions of sodium and chlorine, which now allow the solution to conduct electricity through its positive and negative charges. So the ionic substance table salt is a strong electrolyte. And that proves that the first attempt didn’t have enough of the ions from NaCl to conduct electricity.
The experiment was repeated using table sugar instead of salt. The term non-electrolyte refers to a substance which dissolves in water but does not allow electrical conductivity. As the sugar dissolves, the light did not light up. So sugar is a non-electrolyte.
Some acids and bases are also strong electrolytes. The next example was
References: eHow.com http://www.ehow.com/about_5039184_ph-stomach-acid.html#ixzz25GXbqItt http://chemistry.about.com/od/chemistryglossary/a/aciddefinition.htm http://en.wikipedia.org/wiki/Acid%E2%80%93base_reaction http://www.chem.purdue.edu/gchelp/howtosolveit/Equilibrium/Calculating_pHandpOH.htm http://idealearthwater.com/faq/what-is-ph-orp Homeostasis - Biology Encyclopedia - cells, body, examples, function, human, process, system, organisms, blood http://www.biologyreference.com/Ho-La/Homeostasis.html#b#ixzz25GrGwjnr http://www.kentchemistry.com/links/AcidsBases/Electrolytes.htm I have observed the conductivity of several substances and of aqueous solutions formed from a number of substances. Based on my observation of conductivity, there were three properties of an electrolyte; strong electrolyte, a weak electrolyte and a nonelectrolyte. I have observed changes in conductivity as far from the progress of the chemical reactions and the prediction of the reaction.