Potassium Iodide Lab

We learning about how ions dissolve in water and also how dissolved ions of different compounds react with each other and finally examine the final product for the presence for ions.

Materials-
Sheet of Paper
Lead (II) Nitrate
Potassium Iodide
Deionized Water
Filter Paper
Charcoal
Matches

Equipment-
Clean dry spatula
Small Beakers
Glass stirring rod
Ring stand
Funnel
Tweezers
Bunsen Burner
Small Test Tubes

Safety-
During this lab we are dealing with some dangerous chemical including Lead Nitrate, Potassium Iodide. In this lab you will need to be wearing safety goggles at all times and closed toed shoes and for people that have long hair they need to have it tied back because we will be using a bunsen burner. Also when handling Lead it
is very dangerous and you need to be extremely careful when handling it and be sure to use spatula at all times. Also when heating chemicals be sure to be aware of where the test tube is pointed towards people in your area and making sure that all of people in the vicinity are a aware of the of this happening.

Data/Observations-

Observations
Lead (ii) Nitrate
Potassium Iodide
Solid (Alone) white, grainy, crystals white, grains (Smaller grains than lead nitrate
Dissolved (Alone) dissolved slowly and looks as clear as water dissolved quickly and also looks as clear as water

Charcoal: Before
Dark and black, smooth chalky block
Charcoal: After
Parts that were covered in the yellow substance turned orange

Reactions
Observations
Mixed
Bright yellow, milky/thick substance
Filtrate
Yellow, solid powder, wet clumps
Test 1
Fire from bunsen burner created yellow and orange smoke and caused charcoal to turn orange
Test 2
The heating of the filtrate in the test tube causes the filtrate to turn orange and it then generates a “black light” purple color smoke

Data Analysis: Not Applicable
Post Lab Questions:
When I put Lead (II) Nitrate and Potassium Iodide in their respective beakers with deionized water, the ions in the two compounds split up. When the Ions split up there where two Nitrate anions, one Lead cation, one Iodine cations, and one Potassium cation. In the solutions the cations will be attracted to negatively charged oxygen atom, and the anions will be attracted to the positive hydrogen atom. But the Lead (II) Iodide was the precipitate so it sunk to the bottom of the solution.
The reason why it is important to use deionized water is because the deionized water is just H2O.
But when you have tap water there is ions from the sink that bond with the wrong elements and this would mess up the conductivity tests.
The Ions that were in the solid product would be our precipitate from out balanced equation. Since we found that Lead (II) Iodide was our precipitate from the solubility rules. These ions were found in the thick yellow solution when we combine both reactants and the precipitate would be found at the bottom. So in conclusion the ions in the solid product would be Pb-2 and I-1.
PbI2
The spectator ions would be found in the solution because they are not part of the solid product. To test to see if the spectator ions are present in the solution would be to conduct a conductivity test. This would work because the the ions conduct electricity and the solid product does not conduct electricity.
The reaction in this lab was a double replacement reaction. Pb(NO3)2(aq) + 2KI(aq) ---> 2KNO3(aq) + PbI2()
7. Net Ionic Equation: Pb+2(aq) + 2I-1(aq)
--->PbI2() Spectator Ions: K+1 and NO3-1
8. This reaction below is a decomposition reaction because it is one compound decomposing in two elements.
PbI2(s) ---> Pb(s) + I2(g)
Conclusion:
In this lab we were trying to accomplish how the dissolved ions of one compound can react with the dissolved ion of another compound to form a precipitate.
In this lab we did complete this lab and accomplish our goal of combining dissolved ions of different compounds to form a precipitate. The data we collected shows that the two reactants we used Lead (II) Nitrate and Potassium Iodide were combined to form the solid product Lead (II) Iodide. The observation we made from this reactions shows how those to reactant reacted to form a thick yellow solid product which was Lead (II) Iodide.
In this lab there were many sources of error that could have affect our experiment. One of this possible errors could have been using a wet or a beaker with another substance inside of it that would have other compounds or residue from other past experiments. This source of error would cause the ions in the solution to dissolve with different compounds and the percent yield would be affected by that. Additionally, leaving some water left behind in the solid product which would leave ions in the solid product and this would ultimately mess up test 1 and test 2 by reacting the wrong
way.
In this lab I experienced many things that I did not know before. For example some of the more interesting things I learned was the reaction of the precipitate from the reaction and charcoal and those too being heated together caused different colors to emerge and cause different color gases which I have never seen before. I also learned in the process of the lab how important using deionized water can be while combing ions.
The content in this lab directly relates to class because in the class we having been learning about molarity and concentration and dilution of substances. In this lab we were combing two diluted solutions to react and form a solid product. Also while writing the balanced equation this relates to previous chapters.