The purpose of this experiment is to become familiar with metal and nonmetal ions and with tests to determine the presence or absence of these important ions as well as to estimate approximate amounts. This experiment is divided into three sections: cations (six tests), anions (four tests), and identification of an unknown salt. For Fe+3 (Iron) test, place about 2 mL of 5% iron(III) chloride (FeCl3) solution in a test tube and add 10% ammonium thiocyanate (NH4SCN) solution until a deep red color appears. Mix the two solutions gently and record the observations on the data sheet. Next is a flame test for Na+1 (Sodium). First, obtain a wire loop and adjust the flame on the burner so that it’s blue. Clean the wire loop by dipping it in concentrated …show more content…
Observe and record. For Ca+2 (Calcium) tests, there is a test for the precipitation and a flame test. First, pour 1 mL of 0.1 M calcium nitrate, Ca(NO3)2, solution into a test tube and add a few drops of 0.1 M sodium oxalate, Na2C2O4, and warm this mixture and mix well, then set it to rest. For the flame test, mix 1 mL of 0.1 M calcium nitrate with a few drops of 6M hydrochloric acid in a test tube and perform a flame test on this solution, same way as the previous flame tests. Next test is for Zn+2 (Zinc): place I mL of 0.1 M zinc nitrate into a test tube and add several drops of 6M ammonium chloride and add 1 drop of 6M ammonium hydroxide and add a few drops of 1 M …show more content…
For NH4+1 (Ammonium Ion) tests, place 2 mL of 0.1 M ammonium nitrate solution in a test tube and add a few drops of 6M sodium hydroxide. Moisten a piece of red litmus paper and hold it at the mouth of the test and gently heat the test tube. When the litmus paper turns blue, cautiously smell the vapor to detect ammonia. After testing the cations, we will test the anions. For Cl-1 (Chloride) test, place 1 mL of 0.1 M sodium chloride solution in a test tube, add a few drops of 0.1 M silver nitrate and verify the presence of the chloride ion by adding 6M ammonium hydroxide in 2-3 drop increments until the precipitate dissolves. Reprecipitate the silver chloride by adding 6M nitic acid until the solution is acid to litmus paper. Observe and record data. For PO4-3 (Phosphate) test, place 1 mL of 0.1 M sodium phosphate in a test tube, add 1 mL of 6M nitric acid and add 1 mL of 0.5M ammonium molybdate and mix thoroughly. Place the test tube in boiling water and remove it after five minutes to observe the solution. For SO4-2 (Sulfate) test, place 1 mL of 0.1 M sodium sulfate in a test tube, add 1 mL of 6M hydrochloric acid, and add 3-4 drops of 0.1M barium chloride and mix
The primary goal of this laboratory project was to identify an unknown compound and determine its chemical and physical properties. First the appearance, odor, solubility, and conductivity of the compound were observed and measured so that they could be compared to those of known compounds. Then the cation present in the compound was identified using the flame test. The identity of the anion present in the compound was deduced through a series of chemical tests (Cooper, 2009).
Fire and thermal properties of PA 66 resin treated with poly-N- aniline- phenyl phosphamide as a flame retardant
This smoke bomb lab helped me understand chemical bonding and reactions by starting from the very beginning with mixing the nitrate, sugar, and melted crayon. Mixing them formed a texture almost like powdery peanut butter with some liquid which was actually pretty interesting. The second chemical bonding I seen was that, once putting the solution in the tin-can and it started solidifying due to all the stuff we mixed together. It didn’t take long at all for it to start forming into a solid. When we went outside and lit the wick on fire showed the main chemical reaction throughout the whole experiment. The nitrate reacting with the lighted wick started a big fire in one of the groups cans but some of the other groups bombs didn’t get to light like it was supposed to and the wick just burned out. I was one of the groups whose bombs didn’t work properly. I think it’s because we didn’t put the wick in deep enough to our solution so when we lit it the fire just burned out before going into the solution.
Solid A was identified to be sodium chloride, solid B was identified to be sucrose, and Solid C was identified to be corn starch. Within the Information Chart – Mystery White Solid Lab there are results that distinguishes itself from the other 4 experimental results within each test. Such as: the high conductivity and high melting point of sodium chloride, and the iodine reaction of corn starch. Solid A is an ionic compound due to its high melting point and high electrical conductivity (7), within the Information Chart – Mystery White Solid Lab there is only one ionic compound which is sodium chloride, with the test results of Solid A, it can be concluded that is a sodium chloride. Solid B was identified as sucrose due to its low electrical
In this To Build A Fire Lab, we had the goal of building a fire with oven mitts on. Vivian and I worked as a team. One person using the oven mitts, and the other person would tell them what they should do. Before this experiment, we read the short story "To Build A Fire", by Jack London. This taught me that we would probably have some trouble building a fire.
When doing the precipitate test of the experiment to figure out anions we have written down qualitative observations, we have also hypothesised that if we cover unknown anion A in Silver Nitrate then it will turn a strong cloudy white because unknown anion A is Potassium Iodide and if we were to cover unknown anion B in Barium chloride then it will go from a transparent aqua/blue to a cloudy light blue because unknown anion B is Copper Sulphate. It is rational to say that we believe the 2 unknown cations are Sodium and Copper while the anions are Iodide and
Experiment: First prepared a well plate with the appropriate amounts of distilled water, HCl, and Na2S2O3 in each well according to the lab manual. The well where the reaction
3.) Divide your 30g of white substance into the 4 test tubes evenly. You should put 7.5g into each test tube along with the water.
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
== § Test tubes X 11 § 0.10 molar dm -3 Copper (II) Sulphate solution § distilled water § egg albumen from 3 eggs. § Syringe X 12 § colorimeter § tripod § 100ml beaker § Bunsen burner § test tube holder § safety glasses § gloves § test tube pen § test tube method = == = =
By doing so, the composition of the material is analyzed, both qualitatively (which components are present in the material) and qualitatively (how much of these components is present). In this experiment, synthesis and thermo gravimetric analysis of calcium oxalate has been carried out. Synthesis of calcium oxalate was done by the reaction between calcium ions and oxalate ion: Ca2+(aq) + C2O42-(aq) arrow CaC2O4(s) In which prepared via precipitation from solution at about pH 5 called homogeneous precipitation. Since calcium oxalate is an oxalic acid, it dissolve in acidic solution, to make the calcium oxalate form precipitate, the solution was adjust to more basic by addition of ammonia, but this is not done by adding the ammonia solution directly into the solution.
1. Obtain a clean, dry crucible and lid, then heat them for approximately 5 minutes over a Bunsen burner
To the first Erlenmeyer flask with the ferrous salt add about 1/3 of the 0.75N sulfuric acid. Dissolve the salt by gently swirling it in the dilute acid. Add about 5mL of the Zimmerman-Reinhardt Reagent (this reagent contains phosphoric acid which complexes yellow ferrous ions into colorless compounds which do not obscure the endpoint; it also contains manganous ions which inhibit the oxidation of any chloride ions in the sample). The use of a white background underneath the flask aids in the detecting of the endpoint. Repeat with second sample.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and