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
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
This paper describes the methods used in the identification, investigation of properties, and synthesis of an unknown compound. The compound was identified as calcium nitrate by a variety of tests. When the compound was received, it was already known to be one of twelve possible ionic compounds. The flame test identified the presence of the calcium anion in the compound. The compound tested positive for the nitrate cation using the iron sulfate test. At this point it was hypothesized that the compound was calcium nitrate. Reactivity tests and quantitative analysis comparing the unknown compound with calcium nitrate supported this hypothesis. Synthesis reactions were then carried out and analyzed.
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.
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
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.
1. Obtain a clean, dry crucible and lid, then heat them for approximately 5 minutes over a Bunsen burner
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.
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.
Conversely, make the ammonia forms slowly within the solution through the reaction of hydrolysis of urea: (H2N)2C =O + H2O arrow 2NH3 + CO2 Urea is a suitable compound in this reaction because it can decomposed easily to form ammonia. During the experiment, the solution was heated after urea has been added in, this is to increase the degree of hydrolysis of urea and therefore increase the formation of ammonia.
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
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.
== § 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 = == = =
Scientific report on cations and anions How can we work out the unknown solutions by completing a flame test and a precipitate test? In this experiment we will work out two different unknown solutions using a flame test and a precipitate test. A flame test is a procedure you use in chemistry, predominantly with a Bunsen burner, to detect certain elements, based on their emission of colour that they give off.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and