Conductivity Of Solutions Lab Conclusion Essay

 

Conductivity Of Solutions

Abstract:

In this experiment, I studied the effect of increasing the concentration of the ioniccompounds NaCl, CaCl

2,

and AlCl

3

on conductivity. Conductivity was measured by graduallyincreasing the concentration by adding drops of the compounds to distilled water.

Procedure/ Lab Materials:

Gathered lab materials: 100mL beaker, stirring rod, ring stand, utility clamp, Data Calculator.

Set up lab materials according to instructions provided in lab.

Added 70mL of dionized water to a 100mL glass beaker.

Gathered a NaCl dropper, a CaCl

2

dropper, and a AlCl

3

dropper.

Activated calculator and connected conductivity probe.

Tested conductivity of water with vernier conductivity probe.

Recorded conductivity of the water and labeled as drop 0.

Added first drop of 8 1.0M NaCl to water.

Stirred solution thoroughly with glass stir rod.

Tested conductivity of the solution with conductivity probe.

Recorded conductivity of 1.0M NaCl on data sheet as drop 1.

Continued adding a drop at a time and testing/recording data for 1.0M NaCl.

After 8

th

drop of NaCl was tested and recorded, cleaned probe and beaker.

Refilled 100mL beaker with 70mL of deionized water.

Tested conductivity of deionized water and recorded as drop 0 for 1.0M CaCl

2.

Repeated steps and tests from 1.0M NaCl for 1.0M CaCl

2.

After 8

th

drop of CaCl

2

was tested and recorded, cleaned probe and beaker.

Refilled 100mL beaker with 70mL of deionized water.

Tested conductivity of deionized water and recorded as drop 0 for 1.0M AlCl

3.

Repeated steps and tests from 1.0M CaCl

2

for 1.0M AlCl

3.

After 8

th

drop of AlCl

3

was tested and recorded, cleaned probe and beaker.

Put up lab equipment and cleaned lab area.

Analysis:

The experiment showed that the conductivity increased as concentration increased. Also,when there are more ions in solution, the conductivity increases such as when aluminum chloridehas a higher conductivity value than calcium chloride and sodium chloride even though theconcentrations are the same. I learned that the more ions a compound has the more conductive it is,aluminum chloride has four ions, sodium chloride has two ions and calcium chloride has threeions, therefore aluminum chloride is the best conductor.2Dzierewienko

Essay about Conductivity Lab

1618 WordsSep 26th, 20127 Pages

Post-Lab Questions 1. Using the information provided in the Introduction and your observations from Part 1, hypothesize as to the type of electrolyte the following solutions would be. Justify the hypothesis from a chemical standpoint. a. Aqueous Sodium Hydroxide—NaOH (aq) is a very strong base, which will completely disassociate into Na+ and OH- ions, which would make it a very strong electrolyte. Chemical reaction of the disassociation of Sodium Hydroxide: NaOH (aq)Na+ (aq)+ OH-(aq) b. Aqueous NaCl—Sodium Chloride contains both sodium and chloride ions, but in the solid state they are locked in place and therefore unavailable to conduct electricity. But, when NaCl is dissolved in water, the ions are free to move and conduct…show more content…

The conducting species at equivalence point would be the Sodium as it has the most free-range electrons and dissociates readily in solutions.4 3. How could a conductometric titration be used to determine the molarity of either reacting solutions, assuming the concentration of one solution was known? HINT: Consider the variables needed to calculate molarity, and how can these values be obtained from the titration. The symbol M stands for molarity with units of mol/L. Molarity is a measure of the concentration of a solution. If you knew the concentration of one of the solutions, the molarity could be found in this way. The concept plan would go as follows: Volume of Titrant (in liters) x Moles of Titrant (mol) = moles of the unknown, and then take Moles of the unknown / Liters of the unknown to get the Molarity of the unknown in mol/L. 4

4. What are the benefits of using a light bulb as an indication of conductivity? What are the disadvantages? The benefits are: it acts as a confident and direct way of determining whether a solution should be classified as strong, weak, or non-electrolyte. A strong light would indicate a strong electrolyte. A dim light indicates a weak electrolyte, and no light indicates a non-electrolyte. However, the disadvantages are the lack of accuracy in each reading, and conclusions that aren’t necessarily precise. Each reading displays a different level of light for each bulb. Therefore, conductivity

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