Electrolytes Lab Report

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Northeastern University *

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2313

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Chemistry

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Apr 3, 2024

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pdf

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3

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Electrolytes Lab Report Introduction: This experiment deals with whether several known compounds are electrolytes. The strength of an electrolyte is determined by the brightness of a light that is produced. A bright light is associated with a strong electrolyte and no light is a nonelectrolyte. Using a circuit, one can observe the strength of the electrolyte based on the strength of the light. Chemical Responsibility: One must wear safety goggles, a lab coat, gloves, and close-toed shoes to protect the skin and the eyes of any chemical particles. This experiment deals with electrical currents so there is a hazard of electrical shock and the parts of the apparatus that carry an electrical shock should not be touched. The salts must be disposed of in the waste salt solutions. The acid and bases must be disposed of in the waste acid-base container. The sugar and alcohol must be disposed of in the waste sugar/alcohol bottle. Lastly, the dilution solution can be poured down the drain. Report Sheet: NaCl = Strong electrolyte CaCl2 = Strong electrolyte NH4Cl = Strong electrolyte 3 M HCl = Strong electrolyte 3 M NaOH = Strong electrolyte 3 M acetic acid = Weak electrolyte 3 M ammonia = Weak electrolyte Upon mixing the acetic acid and ammonia = Strong electrolyte Sugar = nonelectrolyte Alcohol = nonelectrolyte Dilution Effects: NaCl(before dilution) = strong After adding 100mL H20 = strong but not as initial After adding 200mL H20 = weaker than before After adding 300mL H20 = weak light is barely there After adding 400mL H20 = weak there's a faint light After adding 500mL H20 = Super weak there’s still a little bit of light After adding 600mL H20 = extremely weak
Post Lab Question: 1.) Although ammonia and acetic acid themselves are weak electrolytes, a mixture of these two solutions behaved as a strong electrolyte. Why? When ammonia mixes with acetic acid it makes ammonium acetate which is highly soluble in water and will ionize completely to form ammonium and acetate ions. This increases the number of ions in the solution creating a strong electrolyte. 2.) Write the reaction that occurs when ammonia and acetic acid are mixed. CH3CO2H + NH5 -> CH3CO2- + NH4+ 3.) In one portion of this experiment you added a pinch of NaCl to a beaker, and you added progressively more and more water to the beaker. Explain why the light gets dimmer and dimmer. This happens because as there is more water added, there is much more distance between the sodium ions and the chloride ions. This makes the solution not conduct electricity very well making it weaker electrolyte. 4.) You are given three bottles labeled a, b, and c. The bottles contain pentane, calcium chloride solution, and aqueous ammonium hydroxide. Describe a procedure to identify which liquid would be in each bottle. Since pentane is the only solution that is flammable a combustion test could be done to see which bottle has pentane. To test calcium chloride and ammonium hydroxide a pH test can be done since calcium chloride is acidic and ammonium hydroxide is basic. 5.) The deceive used in this experiment only measured the relative conductivity of the solution tested, that is, whether the solution contained a strong, weak or non-electrolyte. A more elaborate conductivity meter can determine a numerical value that can be related to the number of ions in solution. Arrange the following 0.1M solution in order of increasing conductivity and explain why you chose this order. 0.1M glucose = no ions 0.1M NaCl = fewest ions 0.1M MgCl2 = next most ions 0.1M FeCl3 = most ions Discussion of Results: The strength of the electrolyte was determined based on the brightness of the light. The salts (ex. CaCl2) are strong electrolytes as they are completely ionized when placed in water and are highly soluble. HCl is a strong acid and NaOH is a strong base making them strong electrolytes. For the dilution effect, the electrolyte became weaker and weaker as more water was added. This is due to the distance between the ions in the water. These results are
accurate as salts are known to be strong electrolytes and ammonia and acetic acid are known to be weak unless mixed together. Lastly, the more diluted a salt is the weaker the electrolyte. Conclusion: The results support the fact that NH4Cl, CaCl2, and 1M HCl are strong electrolytes as there was a bright light that was produced. 1 M NaOH is a strong base which also produces a bright light. 3 M ammonia and 3 M acetic acid are weak electrolytes as they are weak bases, however the mixture is a strong electrolyte. Both alcohol and sugar were proven to be non-electrolytes as no light was produced. As more water was added the ions were further apart until it was a non-electrolyte.
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